The volume of O2 that can be released at STP from the given sample of silver oxide is 23.45 mL.
To solve this problem
Creating the balanced chemical equation for the breakdown of silver oxide is the first step in tackling this issue:
2Ag2O(s) → 4Ag(s) + O2(g)
We can deduce from the equation that 2 moles of AgO will result in 1 mole of O2. Since Ag2O has a molar mass of 231.735 g/mol, 0.4856 g of Ag2O is equivalent to:
0.4856 g Ag2O x (1 mol Ag2O/231.735 g Ag2O) = 0.002095 mol Ag2O
Therefore, the number of moles of O2 that can be produced from 0.4856 g of Ag2O is:
0.002095 mol Ag2O x (1 mol O2/2 mol Ag2O) = 0.0010475 mol O2
1 mole of any gas takes up 22.4 L of space at STP As a result, 0.4856 g of Ag2O can generate the following amount of O2 at STP:
0.0010475 mol O2 x 22.4 L/mol = 0.02345 L or 23.45 mL
Therefore, the volume of O2 that can be released at STP from the given sample of silver oxide is 23.45 mL.
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The 500 cm³ of a pas enclosed in a container under a pressure of 580 mm of Hg. If the volume is reduced to 300 cm³ what will be the pressure then?
Answer:
The answer is 966.67 mm of Hg.
Explanation:
To solve this problem, we can use Boyle's Law which states that the pressure of a gas is inversely proportional to its volume when the temperature and the amount of gas are kept constant. The formula for Boyle's Law is:
P1V1 = P2V2
where P1 is the initial pressure, V1 is the initial volume, P2 is the final pressure, and V2 is the final volume.
Using the given values:
P1 = 580 mmHg
V1 = 500 cm³
V2 = 300 cm³
We can solve for P2:
P1V1 = P2V2
580 mmHg x 500 cm³ = P2 x 300 cm³
290,000 mmHg·cm³ = P2 x 300 cm³
P2 = 290,000 mmHg·cm³ / 300 cm³
P2 = 966.67 mmHg (rounded to the nearest hundredth)
Therefore, the pressure when the volume is reduced to 300 cm³ is approximately 966.67 mmHg.
What is the difference between practical work inside a laboratory and outside a laboratory
Answer:
The main difference between practical work inside and outside a laboratory is that the practical work inside the lab includes good equipment and chemicals which are very advanced and the practical outside a laboratory is more about the safety of life.
Explanation:
Practicals are set up at stations with lab equipment and chemicals, where students can learn, and researchers can experiment and find different new things.
Thus, the practical work inside the lab includes lab equipment and chemicals, and the practical outside a laboratory is more about conserving nature.
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A gas sample originally occupies 436 mL at 24 C. When the volume is expanded to 612 mL and the temperature is increased to 97 C, the pressure becomes 526 mm Hg. What was the original pressure?
Initially, there was a 266.8 mm Hg pressure.
solve this problem, we can use the combined gas law, which relates the pressure, volume, and temperature of a gas sample. The formula is:
(P1 × V1) ÷ (T1) = (P2 × V2) ÷ (T2)
where P1 and P2 are the initial and final pressures, V1 and V2 are the initial and final volumes, and T1 and T2 are the initial and final temperatures.
We are given that:
- V1 = 436 mL
- V2 = 612 mL
- T1 = 24 C + 273.15 = 297.15 K (convert from Celsius to Kelvin)
- T2 = 97 C + 273.15 = 370.15 K
- P2 = 526 mm Hg
We want to find P1, the original pressure.
Plugging in the values, we get:
(P1 × 436 mL) ÷ (297.15 K) = (526 mm Hg × 612 mL) ÷ (370.15 K)
Solving for P1, we get:
P1 = (526 mm Hg × 612 mL × 297.15 K) ÷ (436 mL × 370.15 K) = 266.8 mm Hg
Therefore, the original pressure was 266.8 mm Hg.
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1. Which of the following stars has a temperature of approximately 9000 K and luminosity about to
20 times greater than the Surfs luminos
a Sirius
b. Procyon
c. Figel
d. Polaris
2. Which of the following types of stars is considered part of the main sequera
a Supergants
b. Red giants
c. Red dwarts
d. White dwarfs
3. Which of the following stars is cooler than the
Surf
a. Procyon B
b. Pigel
C. Barnard's Star
d. Sirius
4. The Sun is classified with which of the following types of stars?
a. Supergiants
b. Red giants
c. Main sequence
d. White dwars
5. Which of the forces listed below is most responsible for the formation of start?
a. Gravity
b. Magnetism
c. Bectromagnetism
d. Light
6. Which star has a higher luminosity and a lower temperature than the Sun?
a. Pigel
b. Barnard's Star
c. Alpha Centauri
d. Aldebaran
7. Compared to the temperature and luminosity of the star Polars, the star Srus is
a. hotter and more luminous
b. hotter and less luminous
c. cooler and more luminous cooler and less luminous
1. The star that has a temperature of approximately 9000 K and luminosity about 20 times greater than the Sun’s luminosity is Vega.
2. The type of star that is considered part of the main sequence is red dwarfs.
3. The star that is cooler than the Sun is Barnard’s Star.
4. The Sun is classified as a main sequence star.
5. The force most responsible for the formation of stars is gravity.
6. The star that has a higher luminosity and a lower temperature than the Sun is Aldebaran.
7. Compared to the temperature and luminosity of the star Polaris, the star Sirius is hotter and more luminous.
Chemistry. . . Reaction: AB₂C (g) → B₂ (g) + AC (g), find the value of K
At equilibrium [AB₂C]=0.0168 M, [B₂]= 0.007 M, and [AC] = 0.0118 M
The value of K at equilibrium, for the reaction is 0.0049
How do i determine the value of K at equilibrium?First, we shall list out the given parameters from the question. This is shown below:
AB₂C (g) ⇌ B₂(g) + AC(g) Concentration of AB₂C, [AB₂C] = 0.0168 MConcentration of B₂, [B₂]= 0.007 MConcentration of AC, [AC] = 0.0118 MEquilibrium constant (K) =?Equilibrium constant is defined as:
Equilibrium constant = [Product]ᵐ / [Reactant]ⁿ
Where
m is the coefficient of productsn is the coefficient of reactantsWith the above formula, we can obtain the equilibrium constant, K as follow:
Equilibrium constant, K = [B₂][AC] / [AB₂C]
K = (0.007 × 0.0118) / 0.0168
K = 0.0049
Thus, the equilibrium constant, K for the reaction is 0.0049
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Why is leaf called the kitchen of the plant?
Plants rely on their leaves to produce food through a process called photosynthesis. This involves converting light energy into organic compounds, like sugars, using chloroplasts that contain the pigment chlorophyll. By combining carbon dioxide and water with light energy, plants create glucose, which serves as an energy source and building material. Along with stomata, which help regulate gas exchange with the environment, the leaf acts as the plant's primary kitchen for food production.
How much aluminum can be produced from 9.00 ton of Al2O3?
To calculate the amount of aluminum produced from 9.00 tons of Al2O3, we need to use stoichiometry. First, we'll convert the mass of Al2O3 to moles, and then use the balanced chemical equation to find the moles of aluminum. Finally, we'll convert the moles of aluminum back to mass.
1. Convert mass of Al2O3 to moles:
9.00 tons = 9,000 kg
Molar mass of Al2O3 = (2 * 26.98) + (3 * 16.00) = 101.96 g/mol
9,000 kg * (1000 g/kg) = 9,000,000 g
moles of Al2O3 = 9,000,000 g / 101.96 g/mol = 88,258 moles
2. Use balanced chemical equation to find moles of aluminum:
The balanced chemical equation is:
2 Al2O3 → 4 Al + 3 O2
Using stoichiometry, we find the ratio of Al2O3 to Al is 2:4 or 1:2.
moles of Al = 88,258 moles Al2O3 * (2 moles Al / 1 mole Al2O3) = 176,516 moles
3. Convert moles of aluminum back to mass:
Molar mass of Al = 26.98 g/mol
Mass of Al = 176,516 moles * 26.98 g/mol = 4,762,984 g
Mass of Al in tons = 4,762,984 g / (1000 g/kg) / (1000 kg/ton) = 4.76 tons
So, 4.76 tons of aluminum can be produced from 9.00 tons of Al2O3.
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Question 6 (5 points)
Label each situation as metals, nonmetals, or metalloids. Label each with numbers.
Usually conducts electricity
& heat well
at room temperature these
are gases or liquids
Will lose valance electrons
to form compounds.
can be used as
semiconductors
Will gain valance electrons
to form compounds.
1. a metal
2. a nonmetal
3. a metalloid
Answer:
Explanation:
Here are the labels for each situation:
1.Usually conducts electricity & heat well - Metal (1)
2.At room temperature these are gases or liquids - Nonmetal (2)
3.Will lose valance electrons to form compounds - Metal (1)
4.Can be used as semiconductors - Metalloid (3)
5.Will gain valance electrons to form compounds - Nonmetal (2)
what is the ph of a .100M naclo solution
The pH of a 0.100M NaClO solution is 1.
How to calculate pH?pH, meaning power of hydrogen, is a measure of how acidic/basic a solution is. The range goes from 0 - 14, with 7 being neutral. pHs of less than 7 indicate acidity, whereas a pH of greater than 7 indicates a base.
pH is really a measure of the relative amount of free hydrogen and hydroxyl ions in the water. It can be estimated using the following formula;
pH = - log {H+}
Where;
H+ = hydrogen ion concentrationpH = - log {0.100}
pH = 1
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Pleas help!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
_______________________________
2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2(g)
Moles of NA = Given Mass (g) ÷ Molecular Mass (g/mol)
= 27.5 ÷ 22.9897
= 1.196 mol
Moles of H2 Produced = Mol of NA × 1 mol H2 ÷ 2 Mol NA
= 1.196 × 1 ÷ 2
= 0.60 mol
Number of Molecules = Moles × Avogadro's Number
= 0.60 × 6.023 × 10²³ mol - 1
= 3.61 × 10²³
The Number of Molecules of Hydrogen Gas Produced When Added To Water Is 3.61 × 10²³
_________________________________
Aqueous sulfuric acid (H₂SO₂) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium sulfate (Na₂SO) and liquid water (H₂O). What is the
theoretical yield of sodium sulfate formed from the reaction of 4.9 g of sulfuric acid and 5.0 g of sodium hydroxide?
Round your answer to 2 significant figures.
The theoretical yield of sodium sulfate, Na₂SO₄, formed from the reaction of 4.9 g of sulfuric acid, H₂SO₄ and 5.0 g of sodium hydroxide, NaOH is 7.1 g
How do i determine the theoretical yield?First, we shall determine the limiting reactant. This is shown below:
H₂SO₄ + 2NaOH -> Na₂SO₄ + 2H₂O
Molar mass of H₂SO₄ = 98 g/molMass of H₂SO₄ from the balanced equation = 1 × 98 = 98 g Molar mass of NaOH = 40 g/molMass of NaOH from the balanced equation = 2 × 40 = 80 gFrom the balanced equation above,
98 g of H₂SO₄ reacted with 80 g of NaOH
Therefore,
4.9 g of H₂SO₄ will react with = (4.9 × 80) / 98 = 4 g of NaOH
From the above calculation, we can see that only 4 g of NaOH out of 5 g is needed to react with 4.9 g H₂SO₄.
Thus, the limiting reactant is H₂SO₄
Finally, we shall determine theoretical yield of sodium sulfate, Na₂SO₄ formed. Details below:
H₂SO₄ + 2NaOH -> Na₂SO₄ + 2H₂O
Molar mass of H₂SO₄ = 98 g/molMass of H₂SO₄ from the balanced equation = 1 × 98 = 98 gMolar mass of Na₂SO₄ = 142 g/molMass of Na₂SO₄ from the balanced equation = 1 × 142 = 142 gFrom the balanced equation above,
98 g of H₂SO₄ reacted to produce 142 g of Na₂SO₄
Therefore,
4.9 g of H₂SO₄ will react to produce = (4.9 × 142) / 98 = 7.1 g of Na₂SO₄
Thus, the theoretical yield of sodium sulfate, Na₂SO₄ formed is 7.1 g
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Which of these are part of the
Earth's lithosphere?
O clouds
O glaciers
O mountains
O water vapor
Convert the following number
into correct scientific notation.
0.0602 x 10^25
[ ? ] × 10 [ ? ]
The number is converted to 60. 2 × 10²²
What are index forms?Index forms are simply described as mathematical forms that are used in the representation of numbers that are too small or too large in more convenient forms.
These index forms are also referred to as scientific notation or standard forms.
Some rules of index forms are;
Add the exponents when multiplying forms of the same basesSubtract the exponents when dividing forms of the same basesFrom the information given, we have that;
0. 0602 × 10 ²⁵
Subtract three from the exponent value and move three spaces right, we have;
60. 2 × 10²⁵⁻³
60. 2 × 10²²
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If the reaction A (aq) + B (aq) C(aq) has a Ka value equal to 4.26 x 10-6, what is the G value at 25 °C if the concentrations are as follows:
[A] = 1.50 M
[B] = 1.00 M
[C] = 5.00 x 10-5 M
The Gibbs free energy change for the given reaction at 25°C and the given concentrations is -25.5 kJ/mol
The Gibbs free energy change (∆G) of a reaction can be calculated using the equation:
∆G = -RT ln(K)
Where R is the gas constant (8.314 J/molK), T is the temperature in Kelvin, and K is the equilibrium constant.
The equilibrium constant (K) can be calculated from the acid dissociation constant (Ka) as:
K = [C] ÷ ([A] × [B])
Substituting the given values, we get:
K = (5.00 x 10⁻⁵) ÷ (1.50 x 1.00) = 3.33 x 10⁻⁵
Therefore,
∆G = - (8.314 J/molK) × (298 K) × ln(3.33 x 10⁻⁵)
= 25.5 kJ/mol
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using the equation PCI5(g) PCI3(g) + CI2(g), if CI2 is added, what way will the euilibeium shift
When an equilibrium system is put under stress, Le Chatelier's principle can be used to forecast changes in equilibrium concentrations.
Thus, The adjustments required to reach equilibrium might not be as obvious if we have a mixture of reactants and products that have not yet reached equilibrium.
In this situation, we can compare the Q and K values for the system to forecast changes.
By adding or withdrawing one or more of the reactants or products, an equilibrium chemical system can be momentarily moved out of equilibrium. After that, additional adjustments are made to the reactant and product concentrations in order to bring the system back to equilibrium.
Thus, When an equilibrium system is put under stress, Le Chatelier's principle can be used to forecast changes in equilibrium concentrations.
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1. To operate a batch reactor for converting A into R. This is a liquid phase reaction with the stoichiometry A → R. CA,(mol/l) 0.1 0.2 0.3 0.4 0.2 0.6 0.7 0.8 1.0 1.3 2.0 -rA,(mol/l min) 0.1 0.3 0.5 0.6 0.5 0.25 0.10 0.06 0.05 0.045 0.042 For the above data determine the order of reaction and rate constant.
The reaction is second order with a rate constant of 0.043 mol/l min.
How to explain the reactionFor CA = 0.1 mol/l, -rA = 0.1 mol/l min
For CA = 0.2 mol/l, -rA = 0.3 mol/l min
For CA = 0.3 mol/l, -rA = 0.5 mol/l min
For CA = 0.4 mol/l, -rA = 0.6 mol/l min
The slope of this line is equal to the order of the reaction (n), and the y-intercept is ln(k).
Slope = (0.6931 - (-2.3026)) / (0.3010 - (-0.9163)) = 1.929
ln(k) = -2.3026 + 1.929 * (-0.3010)
ln(k) = -3.1504
k = e^(-3.1504) = 0.043 mol/l min
The reaction is second order with a rate constant of 0.043 mol/l min.
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A gas‑filled weather balloon has a volume of 56.0 L
at ground level, where the pressure is 761 mmHg
and the temperature is 23.1 ∘C.
After being released, the balloon rises to an altitude where the temperature is −6.97 ∘C
and the pressure is 0.0772 atm.
What is the weather balloon's volume at the higher altitude?
What happens to a buffered solution when a small amount of base is added?
O The solution quickly becomes neutral.
O The solutions resists changes in pH.
O The solution slowly becomes acidic.
O The solution quickly becomes basic.
Answer:
solution resists changes in pH
Explanation:
the inherent property of buffers is to resist change to ph even when acids and bases are added. when the base is added, it is quickly neutralized by the conjugate acid, so the ph won't change.
Answer:
B: The solutions resists changes in pH.
Explanation:
Buffer reactions maintain stable pH of solutions.
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6 , and an unknown amount of propane, C3H8 ) were added to the same 10.0- L container. At 23.0 ∘C, the total pressure in the container is 3.70 atm. Calculate the partial pressure of each gas in the container.
The partial pressure of each gas are:
Partial pressure of CH₄ is 1.22 atmPartial pressure of C₂H₆ is 1.46 atmPartial pressure of C₃H₈ is 1.02 atmHow do i determine the partial pressure of each gas?First, we shall determine the mole of 8.00 g of methane, CH₄ and 18.0 g of ethane, C₂H₆. Details below:
For methane, CH₄
Mass of CH₄ = 8 g Molar mass of CH₄ = 16 g/mol Mole of CH₄ =?Mole = mass / molar mass
Mole of CH₄ = 8 / 16
Mole of CH₄ = 0.5 mole
For ethane, C₂H₆
Mass of C₂H₆ = 18 g Molar mass of C₂H₆ = 30 g/mol Mole of C₂H₆ =?Mole = mass / molar mass
Mole of C₂H₆ = 18 / 30
Mole of C₂H₆ = 0.6 mole
Next, we shall determine the total mole. Details below:
Volume (V) = 750 mL = 10 LTemperature (T) = 23 °C = 23 + 273 = 296 KPressure (P) = 3.70Gas constant (R) = 0.0821 atm.L/mol KTotal of mole (n) =?PV = nRT
3.70 × 10 = n × 0.0821 × 293
Divide both sides by (0.0821 × 293)
n = (3.70 × 10) / (0.0821 × 293)
n = 1.52 mole
Finally, we shall determine the partial pressure of each gas. Details below:
For methane, CH₄
Mole of CH₄ = 0.5 moleTotal mole = 1.52 moleTotal pressure = 3.70 atmPartial pressure of CH₄ =?Partial pressure = (Mole / total mole) × total pressure
Partial pressure of CH₄ = (0.5 / 1.52) × 3.70
Partial pressure of CH₄ = 1.22 atm
For ethane, C₂H₆
Mole of C₂H₆ = 0.6 moleTotal mole = 1.52 moleTotal pressure = 3.70 atmPartial pressure of C₂H₆ =?Partial pressure = (Mole / total mole) × total pressure
Partial pressure of C₂H₆ = (0.6 / 1.52) × 3.70
Partial pressure of C₂H₆ = 1.46 atm
For propane, C₃H₈
Partial pressure of CH₄ = 1.22 atmPartial pressure of C₂H₆ = 1.46 atmTotal pressure = 3.70 atmPartial pressure of C₃H₈ =?Partial pressure of C₃H₈ = Total pressure - (Partial pressure of CH₄ + Partial pressure of C₂H₆)
Partial pressure of C₃H₈ = 3.7 - (1.22 + 1.46)
Partial pressure of C₃H₈ = 1.02 atm
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A solution contains 0.0400 M Ca2+ and 0.0990 M Ag+. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first?
Ca3(PO4)2
Ag3PO4
Na3PO4
When the second cation just starts to precipitate, what percentage of the first cation remains in solution?
15.66% of the first cation is still in solution as the second cation is just beginning to precipitate.
What is phosphate used for?One of the three main nutrients that are most frequently used in fertilisers is phosphorous, which is obtained from processing phosphate rock (the other two are nitrogen and potassium).
You can also make phosphoric acid into phosphoric acids, which are utilised in everything from food and skincare to animal feed and electronics. Over the course of millions of years, organic matter accumulates to form the sedimentary rock known as phosphate.
When [tex]Na_{3}Po_{4}[/tex] added to the solution of Ca and Mg, [tex]Ca_{3}(Po_{4})_{2}[/tex] and [tex]Ag_{3}Po_{4}[/tex] are formed.
Ksp of [tex]Ca_{3}(Po_{4})_{2} = 2.07*10^{-33}[/tex]
Ksp of [tex]Ag_{3}Po_{4} = 0.09*10^{-17}[/tex]
Concentration of [tex][Ca^{2+}][/tex] = 0.040 M
Concentration of [tex][Ag^{+}][/tex] = 0.0990 M
[tex]Ag_{3} Po_{4} - > 3Ag^{+} + Po_{4}^{3-}[/tex]
Ksp = [tex][Ag^{+}]^{3} [Po4^{3-}][/tex]
[tex]0.09*10^{-17} = (0.099)^{3} [Po_{3-}][/tex]
[tex][Po_{3-}] = 9.16*10^{-14}M[/tex]
[tex]Ksp = [Ca^{2+}]^{3} [Po_{3-}][/tex]
[tex]2.07*10^{-33} = (0.040)^{3} [Po_{4}^{3-}]^{2}[/tex]
[tex][Po_{4}^{3-}] = 5.68*10^{-15} M[/tex]
[tex][Po_{4}^{3-}][/tex] is smaller in [tex]Ca_{3}(Po_{4})_{2}[/tex]
[tex]Ca_{3}(Po_{4})_{2}[/tex] will start precipitating first
[tex]Ksp = [Ca^{2+}]^{3} [Po_{4}^{3-}]^{2}[/tex]
[tex]2.07*10^{-33} = [Ca^{2+}]^{3} (9.16*10^{-14})^{2}[/tex]
[tex][Ca^{2+}] = 6.27*10^{-3} M[/tex]
[tex]\%\ of\ Ca^{2+}[/tex] remaining [tex]= 6.27*10^{-3}/0.040 * 100[/tex]
= 15.66 %
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What is the molar mass of a compound if a gaseous sample has a density of 0.978 g/L at 30 °C and 615 torr? The temperature in Celsius is known to two significant figures.
If a gaseous sample has a density of 0.978 g/L at 30 °C and 615 torr, the molar mass of the compound is 24.8 g/mol.
To calculate the molar mass of the compound, we first need to calculate the number of moles present in the gaseous sample using the ideal gas law:
PV = nRT
Where P is the pressure in atm, V is the volume in L, n is the number of moles, R is the gas constant (0.0821 L atm/mol K), and T is the temperature in Kelvin.
Converting the given pressure of 615 torr to atm:
615 torr = 0.811 atm
Converting the given temperature of 30°C to Kelvin:
30°C + 273.15 = 303.15 K
Rounding off to two significant figures, we get:
P = 0.81 atm
T = 303 K
Now, rearranging the ideal gas law equation to solve for n:
n = PV/RT
Substituting the given values:
n = (0.978 g/L) x (1 L) / (0.081 atm x 0.0821 L atm/mol K x 303 K)
n = 0.0394 mol
Next, we can calculate the molar mass of the compound using the formula:
molar mass = mass / mole
molar mass = (0.978 g/L) x (1 L) / 0.0394 mol
molar mass = 24.8 g/mol
Therefore, 24.8 g/mol is the molar mass of the compound.
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Chromium, Cr, has the following isotopic masses and fractional abundances:
Mass Number Isotopic Mass (amu) Fractional Abundance
50 49.9461 0.0435
52 51.9405 0.8379
53 52.9407 0.0950
54 53.9389 0.0236
What is the atomic mass of chromium
The average mass of chromium is 52.1. Isotopic mass is defined as the average mass of all the isotopes of a specific element.
The average atomic mass of an element is referred to as the sum of the masses of its isotopes, each multiplied by its natural abundance which can be also explained as the decimal associated with the percent of atoms of that element that are of a given isotope. Average atomic mass is equal to f1M1 + f2M2 and so on. Hydrogen, chromium, lithium, cobalt, oxygen, boron, plutonium, and carbon are some examples.
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What is the equilibrium constant, K? 3 A(g) + 3 B(g) <-> 5 C(g) + 2 D(g)
The equilibrium constant is written as;
Keq = [tex][D]^2 [C]^5/[A] [B]^3[/tex]
What is the equilibrium constant?The equilibrium constant's value is influenced by the reaction's chemical make-up and temperature.
The product of the product concentrations, each raised to the power of their stoichiometric coefficient, divided by the product of the reactant concentrations, each raised to the power of their stoichiometric coefficient, is known as the equilibrium constant.
The equilibrium constant is Keq = [tex][D]^2 [C]^5/[A] [B]^3.[/tex]
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What is the molar volume of CO2 at 39 C and 652 torr?
The molar volume of a gas can be calculated using the ideal gas law:
PV = nRT
where P is the pressure of the gas in atmospheres (atm), V is the volume of the gas in liters (L), n is the number of moles of gas, R is the ideal gas constant (0.08206 L·atm/mol·K), and T is the temperature of the gas in Kelvin (K).
To solve for the molar volume of CO2 at 39°C (312 K) and 652 torr (0.859 atm), we can rearrange the ideal gas law as follows:
V = (nRT) / P
First, we need to calculate the number of moles of CO2. We can use the following equation, which relates the pressure, volume, number of moles, and temperature of a gas:
PV = nRT
Solving for n, we get:
n = (PV) / (RT)
Substituting the given values, we get:
n = (0.859 atm * V) / (0.08206 L·atm/mol·K * 312 K)
Now we can substitute this expression for n into the equation for the molar volume:
V = (nRT) / P
V = [(0.859 atm * V) / (0.08206 L·atm/mol·K * 312 K)] * (0.08206 L·atm/mol·K * 312 K) / (0.859 atm)
Simplifying, we get:
V = 24.45 L/mol
Therefore, the molar volume of CO2 at 39°C and 652 torr is 24.45 L/mol.
Here are some data from a similar experiment, to determine the empirical formula of on oxide of tin.
Calculate the empirical formula according to these data.
Mass of crucible, cover, and tin sample 21.76 g
Mass of empty crucible with cover 19.66 g
Mass of crucible and cover and sample,
after prolonged heating gives constant weight 22.29 g
The information given can be used to construct the empirical formula for a tin oxide. We must first determine the mass of tin in the sample. This may be achieved by deducting the mass of the crucible, cover, and sample (21.76 g) from the mass of the empty crucible and cover (19.66 g).
This gives us a mass of 2.10 g of tin in the sample. The mass of oxygen in the sample must then be determined. To achieve this, we must deduct the mass of the crucible, cover, and sample (21.76 g) from the mass of the same components (22.29 g) prior to protracted heating. This provides us with an oxygen mass of 0.53 g.
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Please help thanks so much!!!!!!!!!!!!
The total mass of products obtained when 130 g of zinc react completely with HCl is 274 g (3rd option)
How do i determine the total mass of products obtained?First, we shall determine the mass of each product obtained. Details below:
For ZnCl₂
2HCl + Zn -> ZnCl₂ + H₂
Molar mass of Zn = 65 g/molMass of Zn from the balanced equation = 1 × 65 = 65 g Molar mass of ZnCl₂ = 135 g/molMass of ZnCl₂ from the balanced equation = 1 × 135 = 135 gFrom the balanced equation above,
65 g of Zn reacted to produce 135 g of ZnCl₂
Therefore,
130 g of Zn will react to produce = (130 × 135) / 65 = 270 g of ZnCl₂
Thus, the mass of ZnCl₂ obtained is 270 g
For H₂
2HCl + Zn -> ZnCl₂ + H₂
Molar mass of Zn = 65 g/molMass of Zn from the balanced equation = 1 × 65 = 65 g Molar mass of H₂ = 2 g/molMass of H₂ from the balanced equation = 1 × 2 = 2 gFrom the balanced equation above,
65 g of Zn reacted to produce 2 g of H₂
Therefore,
130 g of Zn will react to produce = (130 × 2) / 65 = 4 g of H₂
Thus, the mass of H₂ obtained is 4 g
Finally, we shall determine the total mass of the product produced. Details below:
Mass of ZnCl₂ = 270 gMass of H₂ = 4 gTotal mass of product =?Total mass of product = mass of ZnCl₂ + mass of H₂
Total mass of product = 270 + 4
Total mass of product = 274 g (3rd option)
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Gaseous butane (CH3(CH2)2CH3) will react with gaseous oxygen (02) to produce carbon dioxide (CO2) and gaseous water (H2O). Suppose 34.g of butane s mixed with 200. g of oxygen. Calculate the maximum mass of water that could be produced by the chemical reaction. Be sure your answer has the correct number of significant digits.
The maximum mass of water that can be produced by the reaction is 43.3 g, rounded to three significant figures.
Determining the maximum mass of water producedThe balanced chemical equation for the reaction between butane and oxygen is:
C4H10 + 13/2 O2 → 4 CO2 + 5 H2O
From the equation, we can see that 1 mole of butane reacts with 13/2 moles of oxygen to produce 5 moles of water.
moles of butane = 34. g / 58.12 g/mol = 0.585 mol
moles of oxygen = 200. g / 32.00 g/mol = 6.25 mol
Determining the limiting reactant.
butane : oxygen = 0.585 mol : 6.25 mol
= 0.0936 : 1.00
stoichiometric ratio = 1 : 13/2
= 0.7692 : 1.00
Since the actual ratio is lower than the stoichiometric ratio for oxygen, it is the limiting reactant.
The maximum amount of water that can be produced is determined by the amount of limiting reactant (oxygen).
moles of water = 5/13 * 6.25 mol
= 2.403 mol
Finally, we can convert the moles of water to grams:
mass of water = 2.403 mol * 18.015 g/mol
= 43.3 g
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Macmillan Learning Determine the formal charge on each atom in the structure. H H-B-H H What is the overall charge on the structure? -2 +1 Answer Bank +2 +3 -3 -4 +4 0
The overall charge on the structure is negative one (-1).
The central boron atom in the structure is bonded to two hydrogen atoms. Boron has three valence electrons, and it has formed only two bonds, so it has a formal charge of +1.
Each of the hydrogen atoms has one valence electron, and each is bonded to the boron atom, so each hydrogen atom has a formal charge of -1. The sum of the formal charges in the structure is equal to the charge of the ion, which is -2. Adding up the formal charges of the atoms, we get:
B: +1
H: -1 (two times)
Overall charge = sum of formal charges = +1 - 1 - 1 = -1
Therefore, the overall charge on the structure is negative one (-1).
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diffrences in water temperature in the ocean create movement because-
Diffrences in water temperature in the ocean create movement because bodies of water at different temperatures have different densities.
How can the differences be explained?Water that is colder is generally denser than water that is warmer, so when a body of water with colder, denser water is next to a body of water with warmer, less dense water, a density gradient is established. This gradient creates a difference in pressure between the two bodies of water, with the colder, denser water being at a higher pressure than the warmer, less dense water.
This difference in pressure creates a force that drives the movement of water from the denser, colder region to the less dense, warmer region. This movement of water is known as convection, and it can occur both vertically and horizontally in the ocean. Vertical convection occurs when differences in temperature cause water to rise or sink, while horizontal convection occurs when water moves laterally due to differences in temperature.
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missing options:
1. as water heats up, the atoms of water more faster.
2. warm water is pulled more by gravity than cold water.
3. warm and cold water mix and reach the same temperature.
4. bodies of water at different temperatures have different densities.
A specific organic reaction is described by the energy diagram drawn below. Using this
energy diagram, identify which product will form first and which product will be the
major product if given enough time?
The product that is formed first is product B and the product that will be the major product if given enough time would also be product B.
In an energy diagram, the vertical axis represents the overall energy of the reactants, while the horizontal axis is the ‘reaction coordinate’, tracing from left to right the progress of the reaction from starting compounds to final products.
The activation energy of the reaction can be shown on a diagram as the energy between the reactants that the transition state.
The product with lesser activation energy is the product that is formed first and the major product is decided by the stability of the product which depends on the energy. Lesser is the energy of the product, greater is its stability.
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