Answer: -204.48 celsius
Explanation:
Gay lussac law P1/T1 = P2/T2
T2 = T1P2/P1
I AM ASSUMING THAT 1.92 IS IN ATMS
Temperature must be in Kelvin
t2= 292.15 x 0.45/1.92 =68.47 K
68.47-273.15 = -204.48 celsius it is a negative number
How many liters of a 3.58 MK2SO4 solution are needed to provide 85.1 g of K2SO4 (molar mass 174.01g/mol)? Recall that M is equivalent to mol/L.
Explanation:
Conservation of Mass In chemical reactions, mass is neither gained nor lost. The total mass of all the reactants equals the total mass of all the products. Atoms are just rearranged into different compounds. Using this idea, solve the following problems. 1. 2KCIO3 2KCI+ 30₂ If 500 g of KCIO, decomposes and produces 303 g of KCI, how many grams of O₂ are produced? 2. N₂ + 3H₂ 2NH3 How many grams of H₂ are needed to react with 100 g of N₂ to produce 121 g of NH₂? 3. 4Fe +30₂ 2Fe₂O3 How many grams of oxygen are needed to react with 350 g of iron to produce 500 g of Fe₂O3? 4. CH₂ + 20₂2 CO₂ + 2H₂O 16 g of CH₂ react with 64 g of O₂, producing 44 g of CO₂ How many grams of water are produced? 5. CaCO3 Cao + CO, How much CO, is produced from the decomposition of 200 g of CaCO, if 112 g of CaO are produced?
Answer:
1. The balanced equation is 2KCIO3 → 2KCI + 3O2. According to the law of conservation of mass, the mass of the reactants must equal the mass of the products. Therefore, the mass of oxygen produced is:
Mass of oxygen = Mass of KCIO3 - Mass of KCI
Mass of oxygen = 500 g - 303 g
Mass of oxygen = 197 g
Therefore, 197 g of O2 are produced.
2. The balanced equation is N2 + 3H2 → 2NH3. We need to find out how much H2 is needed to react with 100 g of N2 to produce 121 g of NH3. First, we need to calculate the number of moles of N2 and NH3:
Moles of N2 = Mass of N2 / Molar mass of N2
Moles of N2 = 100 g / 28 g/mol
Moles of N2 = 3.57 mol
Moles of NH3 = Mass of NH3 / Molar mass of NH3
Moles of NH3 = 121 g / 17 g/mol
Moles of NH3 = 7.12 mol
According to the balanced equation, 1 mole of N2 reacts with 3 moles of H2 to produce 2 moles of NH3. Therefore, the number of moles of H2 needed is:
Moles of H2 = Moles of N2 x (3/1)
Moles of H2 = 3.57 mol x 3
Moles of H2 = 10.71 mol
Finally, we can calculate the mass of H2 needed:
Mass of H2 = Moles of H2 x Molar mass of H2
Mass of H2 = 10.71 mol x 2 g/mol
Mass of H2 = 21.42 g
Therefore, 21.42 g of H2 are needed.
3. The balanced equation is 4Fe + 3O2 → 2Fe2O3. We need to find out how much oxygen is needed to react with 350 g of Fe to produce 500 g of Fe2O3. First, we need to calculate the number of moles of Fe and Fe2O3:
Moles of Fe = Mass of Fe / Molar mass of Fe
Moles of Fe = 350 g / 55.85 g/mol
Moles of Fe = 6.26 mol
Moles of Fe2O3 = Mass of Fe2O3 / Molar mass of Fe2O3
Moles of Fe2O3 = 500 g / 159.69 g/mol
Moles of Fe2O3 = 3.13 mol
According to the balanced equation, 4 moles of Fe react with 3 moles of O2 to produce 2 moles of Fe2O3. Therefore, the number of moles of O2 needed is:
Moles of O2 = Moles of Fe x (3/4)
Moles of O2 = 6.26 mol x (3/4)
Moles of O2 = 4.69 mol
Finally, we can calculate the mass of O2 needed:
Mass of O2 = Moles of O2 x Molar mass of O2
Mass of O2 = 4.69 mol x 32 g/mol
Mass of O2 = 150.08 g
Therefore, 150.08 g of O2 are needed.
4. The balanced equation is CH2 + 2O2 → CO2 + 2H2O. We know that 16 g of CH2 reacts with 64 g of O2 to produce 44 g of CO2. We need to find out how much water is produced. First, we need to calculate the number of moles of CH2 and CO2:
Moles of CH2 = Mass of CH2 / Molar mass of CH2
Moles of CH2 = 16 g / 14 g/mol
Moles of CH2 = 1.14 mol
Moles of CO2 = Mass of CO2 / Molar mass of CO2
Moles of CO2 = 44 g / 44 g/mol
Moles of CO2 = 1 mol
According to the balanced equation, 1 mole of CH2 reacts with 2 moles of O2 to produce 2 moles of H2O. Therefore, the number of moles of H2O produced is:
Moles of H2O = Moles of CH2 x (2/1)
Moles of H2O = 1.14 mol x 2
Moles of H2O = 2.28 mol
Finally, we can calculate the mass of H2O produced:
Mass of H2O = Moles of H2O x Molar mass of H2O
Mass of H2O = 2.28 mol x 18 g/mol
Mass of H2O = 41.04 g
Therefore, 41.04 g of H2O are produced.
5. The balanced equation is CaCO3 → CaO + CO2. We need to find out how much CO2 is produced from the decomposition of 200 g of CaCO3 if 112 g of CaO are produced. First, we need to calculate the number of moles of CaCO3 and CaO:
Moles of CaCO3 = Mass of CaCO3 / Molar mass of CaCO3
Moles of CaCO3 = 200 g / 100.09 g/mol
Moles of CaCO3 = 1.999 mol
Moles of CaO = Mass of CaO / Molar mass of CaO
Moles of CaO = 112 g / 56.08 g/mol
Moles of CaO = 1.999 mol
According to the balanced equation, 1 mole of CaCO3 produces 1 mole of CaO and 1 mole of CO2. Therefore, the number of moles of CO2 produced is:
Moles of CO2 = Moles of CaCO3 x (1/1)
Moles of CO2 = 1.999 mol
Finally, we can calculate the mass of CO2 produced:
Mass of CO2 = Moles of CO2 x Molar mass of CO2
Mass of CO2 = 1.999 mol x 44 g/mol
Mass of CO2 = 87.96 g
Therefore, 87.96 g of CO2 are produced.
cyclohexene and sulfric acid reaction
Cyclohexene and sulfuric acid can react to form a cyclic carbonium ion intermediate, which can then undergo various reactions.
What is the product of the reaction?One common reaction is the addition of a nucleophile, such as water or an alcohol, to form an alcohol product. This reaction is often referred to as acid-catalyzed hydration.
The general reaction mechanism can be summarized as follows:
Protonation of the alkene: The sulfuric acid protonates the alkene double bond, creating a more electrophilic carbocation intermediate.
Formation of a cyclic carbonium ion: The positive charge is then delocalized throughout the cyclohexene ring, forming a cyclic carbonium ion intermediate.
Addition of a nucleophile: A nucleophile, such as water, can then attack the carbon atom of the carbonium ion, forming a new bond and creating an alcohol product.
The overall reaction can be written as follows:
Cyclohexene + H2SO4 + H2O → Cyclohexanol + HSO4-
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Which emission spectrum represents the copper?
A.) Spectrum A
B.) Spectrum B
C.) Spectrum C
Answer:b
Explanation:i just did it
what percentage of air is oxygen?
Answer:
21% percent
Explanation:
Air has small amounts of other gases, such as carbon dioxide,neon, and hydrogen. Oxygen shares some parts of air basically. The highest percentage of oxygen we can breathe is approximately 60℅
An isotope of hydrogen, known as Tritium (hydrogen-3), has a half-life of 12 years. If a sample of tritium was prepared 60 years ago, what was its original mass if its current mass is 0.42 micrograms?
Options for answers:
a.) 1.7mg b.) 13.4mg c.) 6.7mg d.) 26.8mg e.) 3.4mg
The original mass of Tritium (hydrogen-3) was 13.4mg if its current mass is 0.42 micrograms.
The formula for radioactive decay is given by:
N = N0 x (1/2)^(t/T)
where,
N = final number of radioactive atoms
N0 = initial number of radioactive atoms
t = time elapsed
T = half-life of the radioactive substance
Let's substitute the given values into the formula:
0.42 μg = N0 x (1/2)^(60/12)
0.42 μg = N0 x (1/2)^5
0.42 μg = N0 x 1/32
N0 = 0.42 μg x 32
N0 = 13.44 μg
Therefore, the original mass of the tritium sample was 13.44 micrograms.
What is radioactive decay?
Radioactive decay is the process by which an unstable atomic nucleus loses energy by emitting ionizing radiation, such as alpha particles, beta particles, and gamma rays. This process can result in a change in the number of protons and/or neutrons in the nucleus, leading to the transformation of one element into another. The rate of decay is typically characterized by a half-life, which is the time required for half of the atoms in a sample to decay.
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A calorimeter contains 21.0 mL of water at 13.5 ∘C. When 1.70g of X (a substance with a molar mass of 77.0 g/mol) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 25.0 ∘C.
Calculate the enthalpy change, ΔH , for this reaction per mole of X.
Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings.
Express the change in enthalpy in kilojoules per mole to three significant figures.
Enthalpy change, H, for this reaction per mole of X is thus equal to 0 J/mol.
How can the water's temperature in the calorimeter be determined?The amount of heat that the calorimeter, q cal, gains may be calculated using the formula qcal = Ccalt, where t is the change in temperature that the mixture experiences.
The equation: can be used to compute the enthalpy change, H. ΔH = q / n
The heat absorbed by the water can be calculated using the equation:
q1 = m1 x c1 x ΔT1
m1 = 21.0 g = 0.0210 kg (since the density of water is 1.00 g/mL)
c1 = 4.18 J/(g⋅∘C)
ΔT1 = 25.0 ∘C - 13.5 ∘C = 11.5 ∘C
q1 = (0.0210 kg) x (4.18 J/(g⋅∘C)) x (11.5 ∘C) = 1.09 J
The heat absorbed by X can be calculated using the equation:
q2 = m2 x ΔHfus
where m2 is the mass of X and ΔHfus is the enthalpy of fusion of X.
m2 = 1.70 g = 0.00170 kg
ΔHfus = ΔH / n = ΔH / (m2/M)
where M is the molar mass of X.
We can rearrange this equation to solve for ΔH: ΔH = q2 x (m2/M)
With this assumption, we can calculate ΔH as follows:
ΔH = q / n = (q1 + q2) / n
ΔH = (1.09 J + q2) / (0.00170 kg / 77.0 g/mol)
ΔH = (1.09 J + q2) / 0.0000221 mol
The fact that the heat absorbed by X is equal to the heat emitted by the solution can be used to solve for q2: q2 = -q1
Therefore, ΔH = (1.09 J - q1) / 0.0000221 mol
Substituting q1, we get:
ΔH = (1.09 J - 1.09 J) / 0.0000221 mol
ΔH = 0 J/mol
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As cocentration increases the vapor pressure does
As the concentration of a solution increases, the vapor pressure decreases.
What is Raoult's law ?Raoult's law states that the vapor pressure of a solution is proportional to the mole fraction of the solvent present in the solution.
When a solute is added to a solvent, it reduces the mole fraction of the solvent, and therefore the vapor pressure of the solution decreases. This is because the solute molecules occupy space on the surface of the solution, which reduces the number of solvent molecules that can escape into the gas phase, and thus reduces the vapor pressure of the solution.
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Complete question:
As the concentration of a solution increases, the vapor pressure _____
A sample of gas is in a container with a movable piston. The volume in the container is originally 850 ML at a temperature of 467K and a pressure of 11 point 4K PA. What will the new temperature if the volume is expanded to 1125 in El with a new pressure of 99.7 K PA?
If the volume is increased to 1125 in El with a new pressure of 99.7 K PA, the new temperature will be around 808 K.
What transpires to the gas volume in a moveable piston cylinder?Once the piston's pressure has doubled, it goes downward until the gas's pressure and the piston pressure are equal. The gas has now lost half of its original volume. The volume of gas falls to one-fourth of its initial volume if the pressure on the piston is once more increased by a factor of two.
This issue can be resolved using the coupled gas law:
(P1V1) / T1 = (P2V2) / T2
Using the following conversions, we can first change the starting volume to litres and the original pressure to atmospheres (atm):
1 mL = 0.001 L
1 kPa = 0.00987 atm
V1 = 850 mL = 0.85 L
P1 = 11.4 kPa = 0.1126 atm
T1 = 467 K
The new volume and pressure can also be converted to litres and atmospheres:
V2 = 1125 mL = 1.125 L
P2 = 99.7 kPa = 0.984 atm
Now we can plug in the values and solve for T2:
(P1V1) / T1 = (P2V2) / T2
(0.1126 atm * 0.85 L) / 467 K = (0.984 atm * 1.125 L) / T2
T2 = (0.984 atm * 1.125 L * 467 K) / (0.1126 atm * 0.85 L)
T2 = 808 K
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Answer:
548 K
I hope this helps! Cheers ^^
I will give brainly IF CORRECT.
What describes an electrolyte?
Question 1 options:
Substances that prohibit electricity from traveling across a solvent
Substance that gives out ions when dissolved in water, which are able to conduct electricity
A chemical used to combust flames in a laboratory setting
A type of current that is utilized to determine if there is a blockage anywhere in the system
Substance that gives out ions when dissolved in water, which are able to conduct electricity describes an electrolyte.
what is sucrose particle type
Answer: Sucrose is a glycosyl glycoside formed by glucose and fructose units joined by an acetal oxygen bridge from hemiacetal of glucose to the hemiketal of the fructose.
Explanation:
uestion 8 Calculate the percentage by mass of hydrogen in PtCl2(NH3)2 A. 1.558 B. 1.008 c.0.672 D. 0.034 E.2.016
The percentage by mass of hydrogen can be calculated from the problem as 2.016
How do you calculate the mass percent of an atom in a compound?To calculate the mass percent of an atom in a compound, you first need to determine the molar mass of the compound and the molar mass of the atom of interest.
Determine the molar mass of the compound by adding up the atomic masses of all the atoms in the compound.
Determine the number of moles of the atom of interest in one mole of the compound. This is done by dividing the atomic mass of the atom by the molar mass of the compound.
We know that the relative molecular mas of the compound is; 300 g/mol
Then;
Percent by mass of hydrogen is; 6/300 * 100/1
= 2.016%
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Find the initial pH in the titration of 25 mL of 0.44 M HF with 0.3 M NaOH. The Ka value is 6.6e-4
Furthermore, 0.179 M of F- ions are present in the solution.
The original pH approach is what?The ASTM D7946, formally known as Standard Test Procedure for Initial pH (i-pH)-Value of Petroleum Products, can be used to measure the i-pH. This technique, which was first presented in 2014, employs a cutting-edge electrode to detect the intensity of the dissolved acids in lubricants. This is not the case with other kinds of titrations, though.
HF + NaOH → NaF + H2O
HF + NaOH → NaF + H2O
moles of HF = Molarity × Volume (in liters)
moles of HF = 0.44 M × 0.025 L
moles of HF = 0.011 mol
moles of NaOH = moles of HF
moles of NaOH = 0.011 mol
Volume of NaOH = 0.011 mol / 0.3 M
Volume of NaOH = 0.037 L or 37 mL
moles of NaOH = 0.3 M × 0.037 L
moles of NaOH = 0.0111 mol
The moles of NaOH remaining after the reaction is:
moles of NaOH remaining = moles of NaOH added - moles of NaOH reacted
moles of NaOH remaining = 0.0093 mol (rounded to 3 significant figures)
[OH-] = Molarity of NaOH
[OH-] = 0.3 M
moles of NaF = moles of NaOH reacted
moles of NaF = 0.0111 mol (rounded to 3 significant figures)
Concentration of NaF = moles of NaF / Volume of solution (in liters)
Volume of solution = Volume of HF + Volume of NaOH added
Volume of solution = 0.025 L + 0.037 L
Volume of solution = 0.062 L
Concentration of NaF = 0.0111 mol / 0.062 L
Concentration of NaF = 0.179 M
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50 points
Problem 1. What masses of 15% and 20% solutions are needed to prepare 200 g of 17% solution?
Problem 2. What masses of 18% and 5% solutions are needed to prepare 300 g of 7% solution?
Problem 3. 200 g of 15% and 350 g of 20% solutions were mixed. Calculate mass percentage of final solution.
Problem 4. 300 g of 15% solution and 35 g of solute were mixed. Calculate mass percentage of final solution.
Problem 5. 400 g of 25% solution and 150 g of water were mixed. Calculate mass percentage of final solution.
80 g of 15% solution and 120 g of 20% solution are needed to prepare 200 g of 17% solution.
What is Mass Percentage?
Mass percentage is the percentage of the mass of the solute in a solution to the total mass of the solution. It is calculated by dividing the mass of the solute by the total mass of the solution and multiplying by 100%. The mass percentage is often used in chemistry to express the concentration of a solution.
Let x be the mass of the 15% solution needed and y be the mass of the 20% solution needed to prepare 200 g of 17% solution. Then we have the system of equations:
x + y = 200 (total mass of the solution)
0.15x + 0.20y = 0.17(200) (total amount of solute in the solution)
Solving for x and y, we get:
x = 80 g of 15% solution
y = 120 g of 20% solution
Therefore, 80 g of 15% solution and 120 g of 20% solution are needed to prepare 200 g of 17% solution.
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The mass of a hydrate is 12.75g. The hydrate is heated and the resulting mass of the
anhydrate is 9.87g. Calculate the experimental percentage of water by mass.
The experimental percentage of water by mass, given that the hydrate is heated and it produces 9.87 g of anhydrous, is 22.6%
How do i determine the experimental percentage of water?First, we shall determine the mass of the water in the hydrate. Details below:
Mass of hydrate = 12.75 gMass of anhydrous = 9.87 gMass of water = ?Mass of water = Mass of hydrate - Mass of anhydrous
Mass of water = 12.75 - 9.87
Mass of water = 2.88
Finally, we shall determine the experimental percentage of water by mass. Details below:
Mass of water = 2.88Mass of hydrate = 12.75 gExperimental percentage of water =?Experimental percentage of water = (mass of of water / mass of hydrate) × 100
Experimental percentage of water = (2.88 / 12.75) × 100
Experimental percentage of water = 22.6%
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What is the percent of H in
Ca(С2H302)2?
(Ca = 40.08 g/mol, C = 12.01 g/mol,
H= 1.01 g/mol, O = 16.00 g/mol)
Answer:
3.8%
Explanation:
Ca × 1 = 50
C ×4 = 48
H × 6 = 6
O × 4 = 64
158
6÷158×100% = 3.8%
!!(100 points)!! What is a valence electron? Which elements on the periodic table have the most valence electrons?
Answer:
sulphur has the most valence electron
Answer:
[tex]valence \: electrons \: are \: the \\ electrons \: in \: the \: outermost \\ shell \: or \: energy \: level \: of \: an \: \\ atom. [/tex]
Help please
2.0 mol of Ca(OH)2 are mixed with 2.0 mol of HCl according to the following equation:
Ca(OH)2+2HCl=CaCl2+2H2O
a. Which chemical is in excess and which is limiting reactant?
b. What is the excess in grams?
c.Theoretically, how many moles of H2O will be produced?
Answer:
Explanation:
Limiting is HCl and excess is Ca(OH)2
excess is 296 grams Ca(OH)2
2 moles H2O will be formed
5. The average human requires .66 moles of glucose (C6H1206) per day. How many mole
of CO2 (in the photosynthesis reaction) are required for this amount of glucose? The
photosynthetic reaction is: 6 CO2 + 6 H₂O ---> C6H12O6 + 6 02
Answer: 3.96 moles of CO2 are required in the photosynthesis reaction.
Explanation: The balanced equation for photosynthesis tells us that for every mole of glucose produced, 6 moles of CO2 are required. Therefore, to determine how many moles of CO2 are required for 0.66 moles of glucose, we can set up a proportion:
6 moles CO2 / 1 mole glucose = x moles CO2 / 0.66 moles glucose
Solving for x, we get:
x = (6 moles CO2 / 1 mole glucose) x (0.66 moles glucose / 1) = 3.96 moles CO2
Therefore, to produce 0.66 moles of glucose, 3.96 moles of CO2 are required in the photosynthesis reaction.
How many moles of MgS are in 100.g MgS?
The number or amount of moles of magnesium sulfide in 100g of MgS is 1.774 moles.
How to calculate number of moles?The number of moles in a substance can be calculated by dividing the mass of the substance by its molar mass as follows:
Mole is the base unit of amount of substance i.e. the amount of substance of a system which contains exactly 6.02214076 × 10²³ elementary entities.
no of moles = mass ÷ molar mass
According to this question, 100g of magnesium sulfide is given. The molar mass of magnesium sulfide is 56.38 g/mol.
moles = 100g ÷ 56.38g/mol
moles = 1.774 moles
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A balloon held at 273 K has an initial volume of 2.0 L at 1.0 atm of pressure. If the pressure is increased to 3.5 atm, what is the new volume of the balloon?
Answer: 5.5 atm
Explanation:
If I have 4 moles of a gas pressure of 5.6 atm and a volume of 12 liters what is the temperature
Answer: 204.63 K
Explanation:
Ideal gas law
Pv=nRT
T=PV/nR
T= 5.6 X 12/(4 x0.0821)= 204.63 K
R= ideal gas constant = 0.0821
which statement describes density? Check all that apply
Density is a chemical property of an object.
The density of an object is constant.
Density is a derived unit of measure.
Density is the sum of the mass and volume of an object.
The density of an object determines whether it will sink or float.
Answer:
The density of an object is constant.
Density is a derived unit of measure.
The density of an object determines whether it will sink or float.
pls help!!
Which statement best describes the difference between speed and velocity?
A.
Velocity is plotted on the x-axis of a graph and speed is plotted on the y-axis.
B.
Velocity is related to position but speed is not.
C.
Velocity does not depend on time but speed does.
D.
Velocity has a specific direction but speed does not.
Answer:
option a
Velocity is plotted on the x-axis of a graph and speed is plotted on the y-axis.
If you are relating the levels of organization of the human body to the levels of organization of a city, what would you relate cells to? what would you relate the other levels to?.
The basic units of the human body are called cells, and they carry out specialized tasks to keep the body alive. Cells in a city might be compared to people who perform particular duties and contribute to the general efficiency of the city.
How do you think the degrees of organization in the human body compare to those in the world?Organizational hierarchy is built up from lower levels. Consequently, molecules combine to create molecules, molecules create cells, cells create tissues, tissues create organs, organs create organ systems, and organ systems create beings. The body's next level of organisation. A tissue is made up of related cells with a common purpose. Human tissues can be divided into four categories: epithelial, muscular, nerve, and connective.
How are the human body's structure and function organized, from the simplest to the most complex?The major levels of organisation in the body, from the most basic to the most complex, are atoms, molecules, organelles, cells, tissues, organs, organ systems, and the human body.
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With 14 liters of loratadine we can fill 135 bottles. How many milliliters of loratadine are needed to fill 106 bottles
It will take about 10990 milliliters to fill 106 vials of loratadine.
Rule of three in ChemistryBased on the information in the statement, to obtain the number of milliliters needed to fill 106 vials of loratadine, just construct the following simple rule of three:
14 liters of loratadine - 135 vials
x liters of loratadine - 106 vials
14 * 106 = 135x
1484 = 135x
x ≅ 10.99 liters of loratadine (value rounded to two decimal places).
Note, however, that the statement asks for the volume of loratadine in milliliters. To convert from liters to milliliters, just multiply the value obtained by above 1000:
10.99 * 1000 = 10990 milliliters.
Create a “Chemical Reaction Poster” that will summarize key concepts about chemical reaction. In your poster, include
Definition of chemical reaction and balanced equation
Steps in balancing chemical equation and an example
Types of chemical reaction and an example for each
Picture/images related to chemical reaction
Other related information
Rubric:
Content ……………………25 points
Organization ……….… 25 points
Neatness/Creativity... 15 points
please help so it can bring my grade up
thank you soo much
project*
Answer:
Ca²+O²
Explanation:
The Ca gives out 2 electrons and oxygen gains 2 elctrons
What is the Percentage of Fluorine as F- in a HF (pKa= 3.33 ) solution at pH= 2.33?
Answer: The percentage of fluorine as F- in a HF solution at pH 2.33 is 9.09%.
Emma is examining evidence from a robbery. She hypothesizes that the robber entered the home from the garage, but when she investigates this, she can't find any signs of forced entry or any physical evidence that supports this. What should her next step be?
A.
create another hypothesis
B.
conduct another experiment
C.
draw a conclusion
1. A 32.5-liter balloon holding 3.5 moles of carbon dioxide leaks. If we determine that 2.1 moles of carbon dioxide escaped before the container could be sealed, what is the new volume of the container?
The new volume of the container is approximately 12.96 liters.
What is the new volume of the container?Assuming that the temperature and pressure remain constant, we can use the ideal gas law to solve for the new volume of the container. The ideal gas law relates the pressure, volume, number of moles, and temperature of a gas as follows:
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.To solve for the new volume, we can use the following steps:
Calculate the initial number of moles of carbon dioxide in the container:
n1 = 3.5 moles
Calculate the final number of moles of carbon dioxide in the container:
n2 = 3.5 moles - 2.1 moles = 1.4 moles
Substitute the values for n1, n2, and the initial volume (V1 = 32.5 L) into the ideal gas law and solve for the final volume (V2):
P V1 = n1 R T
P V2 = n2 R T
Dividing the second equation by the first, we get:
V2 / V1 = n2 / n1
Substituting the values for n1, n2, and V1, we get:
V2 / 32.5 L = 1.4 moles / 3.5 moles
Solving for V2, we get:
V2 = (1.4 moles / 3.5 moles) * 32.5 L
V2 = 12.96 L
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