Determine the pressure of N2 under the following conditions.

49.1 g at 16.6°C in 5.80 L

Answer:

Explanation:

The molar mass of magnesium (Mg) is 24.31 grams per mole (g/mol).

Among the given options, the strongest acid is HClO3 so, it will have the smallest pH. therefore, option d is correct. The pH of a solution is related to the concentration of H+ ions in the solution, with lower pH values corresponding to higher H+ concentrations.

HClO3 is a strong acid that dissociates completely in water, producing H+ and ClO3- ions. Therefore, a 0.1 M HClO3 solution will have a pH of:

pH = -log[H+]

[H+] = 0.1 M (because HClO3 is a strong acid and dissociates completely)

pH = -log(0.1) = 1

On the other hand, the other options are:

a. 0.1 M KOH: This is a strong base that will produce OH- ions in water. However, the concentration of OH- ions is much lower than that of H+ ions produced by HClO3. Therefore, the pH of a 0.1 M KOH solution will be higher than 7, and therefore, it will not have the smallest pH among the given options.

b. 0.1 M CH3NH2: This is a weak base that will produce some OH- ions in water. However, the concentration of OH- ions produced will be much lower than that of H+ ions produced by HClO3. Therefore, the pH of a 0.1 M CH3NH2 solution will be greater than 7, and therefore, it will not have the smallest pH among the given options.

c. 0.1 M CF3COOH: This is a weak acid that will produce some H+ ions in water. However, the concentration of H+ ions produced will be much lower than that of H+ ions produced by HClO3. Therefore, the pH of a 0.1 M CF3COOH solution will be greater than 1, and therefore, it will not have the smallest pH among the given options.

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Answer:

Metals tend to give away electrons during chemical reactions.

Explanation:

This is due to the number of valence electrons held by their atoms.

Answer:

When metals react with other elements, the atoms of the metals lose electrons. This is because metals tend to have low electronegativity, meaning they have a tendency to give up electrons in order to achieve a stable configuration. When they react with other elements, such as nonmetals, the metal atoms will transfer electrons to the nonmetal atoms, forming ionic bonds. The metal atoms become positively charged ions (called cations) because they lose electrons, while the nonmetal atoms become negatively charged ions (called anions) because they gain electrons. This transfer of electrons results in the formation of a compound composed of oppositely charged ions.

Answer:

a single word

Explanation:

Phrase by definition is a group of of words that can stand together. "planted" is the verb used here. It is a single word.

Hydrogen gas and aluminum chloride (AlCl3) is produced when aluminum (Al) and hydrochloric acid (HCl) combine.

When aluminum reacts with hydrochloric acid, hydrogen gas, and aluminum chloride are produced. The reaction is represented by the following chemical equation:

2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2(g)

Aluminum atoms could be represented as solid spheres in a particle diagram for this reaction, and hydrochloric acid molecules could be represented as two tiny spheres that symbolize hydrogen (H) and chlorine (Cl) atoms bound together.

The aluminum atoms would disintegrate when the acid was introduced to it, and the hydrogen and chlorine atoms would disintegrate as well.

The hydrogen atoms would then join forces to form hydrogen gas, and the chlorine atoms would join forces with the aluminum atoms to make aluminum chloride.

Aluminum chloride and hydrogen gas molecules would be visible in the ensuing particle diagram.

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Vitamin C drink with 1025 mg of ascorbic acid contains 3.50 × 10^21 molecules of C6H8O6.

What is Molecules?

A molecule is the smallest particle in a chemical element or compound that has the chemical properties of that element or compound. It is made up of two or more atoms that are chemically bonded together. The atoms can be of the same element, as in the case of diatomic molecules like O2 and H2, or they can be different elements, as in the case of water (H2O) or carbon dioxide (CO2).

First, let's calculate the molar mass of ascorbic acid (C6H8O6):

Molar mass of C = 12.01 g/mol

Molar mass of H = 1.008 g/mol

Molar mass of O = 16.00 g/mol

Molar mass of C6H8O6 = (6 × 12.01) + (8 × 1.008) + (6 × 16.00) = 176.12 g/mol

Now we can use the molar mass to convert the given mass of ascorbic acid into moles:

Number of moles = Mass / Molar mass

Mass of ascorbic acid = 1025 mg = 1.025 g

Number of moles of ascorbic acid = 1.025 g / 176.12 g/mol = 0.00582 moles

Finally, we can use Avogadro's number to convert from moles to molecules:

Number of molecules = Number of moles × Avogadro's number

Number of molecules of C6H8O6 = 0.00582 moles × 6.022 × 10^23 molecules/mol = 3.50 × 10^21 molecules

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Answer:

Explanation:

The wavelength (λ) of an electromagnetic wave can be calculated using the formula:

λ = c / f

where c is the speed of light (approximately 3.00 x 10^8 meters per second) and f is the frequency of the wave.

In this case, the frequency (f) is given as 4.88 x 10^8 Hz.

Substituting these values into the formula, we get:

λ = (3.00 x 10^8 m/s) / (4.88 x 10^8 Hz)

Simplifying this expression, we get:

λ = 0.6148 meters

Therefore, the wavelength of the electromagnetic wave with a frequency of 4.88 x 10^8 Hz is 0.6148 meters (or approximately 61.48 centimeters).

Answer:

Molarity is equal to total moles divided by total liters

Explanation:

Molarity =3.458

                            =2305M

               1.500          

Explanation:

The position of this equilibrium will be well to the left because ethanolic acid is a weak acid: This gets a lot more ethanoate ions when sodium ethanoate is added to it.

The position of this equilibrium will be well to the left because ethanolic acid is a weak acid: Much more ethanoate ions are added when sodium ethanoate is added. That will shift the equilibrium's position even more to the left, in accordance with Le Chatelier's Principle.

Being a weaker acid or base, buffers act by neutralising any additional base (OH- ions) or acid (H+ ions) to preserve the moderate pH.

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1. When 6 M NaOH is added drop-wise to a solution of ZnCl2, a white precipitate forms which dissolves to form a colourless solution as excess reagent is added. The observation suggests the formation of a precipitate that is soluble in excess NaOH. This can be explained by the following balanced net ionic equation:

Zn2+ (aq) + 2OH- (aq) → Zn(OH)2 (s)

The white precipitate is zinc hydroxide, which dissolves in excess NaOH to form the soluble complex ion, [Zn(OH)4]2-.

2. When 6 M NH3 is added drop-wise to a solution of Zn(NO3)2, a white precipitate forms which dissolves to form a colourless solution as excess reagent is added. The observation suggests the formation of a precipitate that is soluble in excess NH3. This can be explained by the following balanced net ionic equation:

Zn2+ (aq) + 2NH3 (aq) + 2H2O (l) → Zn(OH)2 (s) + 2NH4+ (aq)

The white precipitate is again zinc hydroxide, which dissolves in excess NH3 to form the complex ion, [Zn(NH3)4]2+.

3. When 6 M NaOH is added drop-wise to a solution of AlCl3, a white precipitate forms which dissolves when 6 M HCl is added. The observation suggests the formation of a precipitate that is soluble in acid. This can be explained by the following balanced net ionic equation:

Al3+ (aq) + 3OH- (aq) → Al(OH)3 (s)

The white precipitate is aluminium hydroxide, which dissolves in acid to form the soluble ion, Al3+. This can be shown by the following balanced net ionic equation:

Al(OH)3 (s) + 3H+ (aq) → Al3+ (aq) + 3H2O (l)

Therefore, the white precipitate formed by adding NaOH to AlCl3 solution is Al(OH)3, which dissolves when HCl is added due to the formation of the soluble Al3+ ion.

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there are approximately 0.54 zeptomoles of air trapped inside the container with the movable piston.

To calculate the number of zeptomoles of air trapped inside the container with the movable piston, we first need to calculate the volume of the container.

Assuming the container is a rectangular prism with a length and height equal to the size of the graphene sheet (3 cm) and a width equal to the thickness of the spacer (15 nm), the volume of the container can be calculated as:

V = lwh = (3 cm)(3 cm)(15 nm) = 1.35 x 10^-5 cm^3

Next, we need to calculate the number of moles of air trapped inside the container. We can use the ideal gas law to do this:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

We know that the pressure inside the container is equal to atmospheric pressure, which is approximately 101325 Pa (or 1 atm). The temperature is not given, but we can assume it is room temperature, which is approximately 298 K. The ideal gas constant is 8.314 J/(mol*K).

Therefore, we can rearrange the ideal gas law to solve for n:

n = PV/RT

Substituting in the values we know:

n = (101325 Pa)(1.35 x 10^-5 cm^3)/(8.314 J/(mol*K) * 298 K)

n = 5.41 x 10^-28 mol

Finally, to convert this to zeptomoles, we multiply by 10^21:

n = 5.41 x 10^-7 zmol

Therefore, there are approximately 0.54 zeptomoles of air trapped inside the container with the movable piston.

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Answer:

Burning magnesium reaction is a highly exothermic and reactive reaction that produces intense heat and bright light. As a result, it can be dangerous if proper safety precautions are not taken, such as wearing protective eyewear and clothing and working in a well-ventilated area. Additionally, the reaction produces magnesium oxide, which can be harmful if inhaled. Therefore, it is not typically performed in a standard chemistry lab, but rather in a specialized setting with trained professionals and proper safety equipment.

Explanation:

The 750 mL sample of drinking water had 0.021 grams of lead in it.

Use the dilution equation C1V1 = C2V2, where C, concentration, can be expressed in molarity, ppm, ppb, etc. assemble the slope for the absorbance–ppm relationship.

We can first convert the lead concentration from ppm to mg/L because 1 ppm is equal to 1 mg/L: 28 ppm = 28 mg/L

Then, we may determine the mass of lead in the sample using the concentration and volume of the water sample:

Mass of lead = Concentration x Volume

Mass of lead = 28 mg/L x 0.75 L

Mass of lead = 21 mg

Finally, we can convert the mass from milligrams to grams:

Mass of lead = 21 mg = 0.021 g

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We can help explain how to analyze histograms and interpret the information related to cell phone sales.

To analyze histograms, follow these steps:
1. Identify the horizontal axis (x-axis), which should represent the store's operating hours.
2. Identify the vertical axis (y-axis), which should represent the number of cell phone sales.
3. Observe the height of the bars in the histogram. Each bar represents the number of cell phone sales within a specific time interval during the store's operating hours.

To match the statements to the histograms, you should consider the following:
- Look for any patterns or trends in the data, such as higher sales during certain time periods.
- Compare the histograms to determine if there are noticeable differences between the three days.
- Identify any outlier data points or unusually high or low sales during specific time intervals.
Once you have analyzed the histograms, you can match the statements to the appropriate histogram by considering the trends and patterns you've observed.

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the solution is 52.3 g (rounded to two decimal places).

We need to know the mass of the iron and sulphur in order to solve for the amount of sulphur involved. 95 grammes make up the iron's bulk. There are 16 grammes of sulphur in total. Hence, 32 grammes of sulphur are used in this reaction.

The correct answer is:

8Fe + S8 → 8FeS

The molar mass of sulfur is 256 g/mol (8 × 32 g/mol), and the molar mass of iron is 56 g/mol.

First, we need to convert the mass of sulfur to moles:

sulphur mass divided by its molar mass yields moles of sulphur.

moles of sulfur = 30.0 g / 256 g/mol

moles of sulfur = 0.1172 mol

According to the balanced equation, 1 mole of sulfur reacts with 8 moles of iron. Therefore, the moles of iron required can be calculated as:

moles of iron = 8 × moles of sulfur

moles of iron = 8 × 0.1172 mol

moles of iron = 0.9376 mol

Finally, we can calculate the mass of iron required using the moles of iron and the molar mass of iron:

Iron's mass is equal to its molar mass and its moles.

mass of iron = 0.9376 mol × 56 g/mol

mass of iron = 52.46 g

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1 mole of H₂SO₄ reacts with 1 mole of Na₂CO₃, the amount of H₂SO₄ used in the titration is also 0.00125 moles.

What is Mole?

In chemistry, a mole is a unit used to measure the amount of a substance. One mole of a substance contains Avogadro's number of particles, which is approximately 6.02 x [tex]10^{23}[/tex] particles. The mass of one mole of a substance is equal to its atomic or molecular weight in grams.

The balanced chemical equation for the reaction between H₂SO₄ and Na₂CO₃ is:

H₂SO₄ + Na₂CO₃ → Na₂SO₄ + H₂O + CO₂

a) The amount of H₂SO₄ used can be calculated from the burette readings. Assuming the average volume of the acid used is 23.5 cm³, and the concentration of the acid is unknown, we can calculate the number of moles of H₂SO₄ used in the titration as follows:

Moles of H₂SO₄ = Volume of H₂SO₄ (in dm³) x Concentration of H₂SO₄

We don't know the concentration of H₂SO₄, so we can't calculate the amount of H₂SO₄ directly from the titration. We need to use the stoichiometry of the balanced equation to relate the amount of H₂SO₄ to the amount of Na₂CO₃ in solution B.

From the balanced equation, we can see that 1 mole of H₂SO₄ reacts with 1 mole of Na₂CO₃. Therefore, the amount of Na₂CO₃ in solution B can be calculated as follows:

Amount of Na₂CO₃ = 0.050 mol/dm³ x 0.025 dm³ = 0.00125 moles

Since 1 mole of H₂SO₄ reacts with 1 mole of Na₂CO₃, the amount of H₂SO₄ used in the titration is also 0.00125 moles.

b) To calculate the concentration of H₂SO₄ in solution A, we can rearrange the equation above:

Concentration of H₂SO₄ = Moles of H₂SO₄ / Volume of H₂SO₄

Substituting the values we have:

Concentration of H₂SO₄ = 0.00125 moles / 0.0235 dm³ = 0.053 mol/dm³

c) From the balanced equation, we can see that 1 mole of H₂SO₄ produces 2 moles of H⁺ ions. Therefore, the number of hydrogen ions in 1 dm³ of solution A is:

Number of H⁺ ions = 2 x Concentration of H₂SO₄

Substituting the concentration of H₂SO₄ we calculated above:

Number of H⁺ ions = 2 x 0.053 mol/dm³ = 0.106 mol/dm³

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The M electrode in the left half-cell will be oxidized since the left half-cell has a higher concentration and will act as the anode. As a result, the M electrode in the right half-cell will be lowered, and the right half-cell will act as the cathode. As a result, the right half-cell's M electrode will be positive.

The given half-cell reactions are:

Left half-cell: M₂(SO4)₃ + 6 e⁻ → 2M

Right half-cell: M₂(SO4)₃ + 6 e⁻ → 2M

Since both half-cell reactions are the same, the cell potential will be zero at equilibrium. Therefore, the voltmeter will show zero voltage.

However, if we assume that the reactions are not at equilibrium, we can use the Nernst equation to calculate the potential difference between the two electrodes:

Ecell = E°cell - (RT/nF)ln(Q)

where:

E°cell = standard cell potential

R = gas constant = 8.314 J/(mol K)

T = temperature in kelvin = 35.0 + 273 = 308 K

n = number of electrons transferred in the reaction = 6

F = Faraday's constant = 96,485 C/mol

Q = reaction quotient = [M]left / [M]right

The standard cell potential for the given reactions is not provided, but since both half-cell reactions are the same, the standard cell potential will be zero.

Plugging in the values, we get:

Ecell = - (RT/nF)ln(Q)

Ecell = - (8.314 J/(mol K) x 308 K / (6 x 96,485 C/mol)) ln(4.50 M / 2.25 mM)

Ecell = - (0.0257 V) ln(2000)

Ecell = 0.103 V

The M electrode in the left half-cell will be oxidized since the left half-cell has a higher concentration and will act as the anode. As a result, the M electrode in the right half-cell will be lowered, and the right half-cell will act as the cathode. As a result, the right half-cell's M electrode will be positive.

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A chemical reaction in which one element replaces another element in a chemical compound is called a "single displacement reaction" or "single replacement reaction".

A chemical reaction in which two or more substances combine to form a new, more complex substance is called a "combination reaction" or "synthesis reaction".

A chemical reaction in which a substance reacts with oxygen to produce thermal and light energy as well as carbon dioxide and water vapor is called a "combustion reaction".

A chemical reaction in which the positive ion on one compound replaces the positive ion of another compound is called a "double displacement reaction" or "double replacement reaction".

A chemical reaction in which one substance breaks down into two or more simpler substances is called a "decomposition reaction".

The Balanced Chemical Equations:

b. 2NaOH + MgSO4 → Na2SO4 + Mg(OH)2

c. 2 Fe2O3 + 6 H2O → 4 Fe(OH)3

d. 2 HgO → 2 Hg + O2

a. 3 Pb(NO3)2 + 2 AlCl3 → 3 PbCl2 + 2 Al(NO3)3

e. 2 C2H6 → 4 CO + 6 H2O

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See transcribed text below

Fill  Column A with the right term from Column B  

Column A

a.

b

C.

d.

e.

Column B

A chemical reaction in which one element replaces another element in a chemical compound.

A chemical reaction in which two or more substances combine to form a new, more complex substance.

A chemical reaction in which a substance reacts with oxygen to produce thermal and light energy as well as carbon dioxide and water vapor.

A chemical reaction in which the positive ion on one compound replaces the positive ion of another compound.

A chemical reaction in which one substance breaks down into two or more simpler substances.

SECTION B: SKILLS

4. Examine each unbalanced chemical equation and classify it by writing the type of reaction it is on the left. Then, balanced each equation. Draw a chemical reaction beside the test title. (3 points each. 15 points total)

Type of Reaction

Unbalanced Chemical Equation - Balance It!

b.

C.

d.

out of

27

Al

+

Oz

2022 2Aho

2NaOH

+

MgSO4

Na2SO4

Y Mg(OH)2

2-Hgo → 2 Hg +

Liet 6H02 y Fe +

2 Fe2O3 + 12H2

O2

C2H6

+ / 02 2

2c02 +

H2O

The 250 mL solution of 0.10 M HCl contains 0.9115 g of HCl in total.

For acid-base reactions, raffination, and pH control, 0.1M hydrochloric acid is frequently employed. Every educational setting can employ this chemical.

Moles of solute (n) / volume of solution Equals molarity (M) (V)

If we rewrite this formula, we obtain:

moles of solute (n) = Molarity (M) x volume of solution (V)

Substituting the given values, we get:

moles of HCl = 0.10 M x 0.250 L = 0.025 moles

The molar mass of HCl, 36.46 g/mol, may be used to determine its mass. The formula is as follows:

mass of solute (m) = moles of solute (n) x molar mass (M)

When we change the values, we obtain:

mass of HCl = 0.025 mol x 36.46 g/mol

= 0.9115 g

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