Question 1

How many milliliters of ozone gas at at 25.0°C and 1.00 atm pressure are needed to react with 45.00 mL of a 0.100 M aqueous solution of KI according to the chemical equation shown below? O₃(g)+ 2 I^-(aq)+ H₂O(l)→ O₂(g)+ I₂(s)+ 2 OH^-(aq) A) 55.0 mL B) 110. mL C) 165 mL D) 220. mL

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Question 2

Consider a container of gas under a particular P,V,T set of conditions.Describe how the pressure would change if the volume were doubled while the absolute temperature was increasing by a factor of two.

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Question 3

A cylinder filled with nitrogen gas at 80°C occupies 6.82 L at 12.00 atm.It is then quickly cooled to 5°C,and the pressure is measured at 4.82 atm.What is the new volume of the cylinder?
A) 6.42 L
B) 17.3 L
C) 3.38 L
D) 13.4 L

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Question 4

What is the total volume of the mixture of hydrogen gas and oxygen gas can be obtained from the electrolysis of 110.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H₂O(l)→ 2 H₂(g)+ O₂(g) A) 74.7 L B) 149 L C) 224 L D) 447 L

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Question 5

How many grams of water are required to produce 5.50 L of hydrogen gas at 25.0°C and 755 mm Hg pressure according to the chemical equation shown below? BaH₂(s)+ 2 H₂O(l)→ Ba(OH)₂(aq)+ 2 H₂(g) A) 2.01 g B) 4.02 g C) 4.07 g D) 8.04 g

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Question 6

A 9.50L cylinder contains a mixture of 138 g Ne and 403 g Cl₂ at 325 K.What is the partial pressure of Cl₂? A) 16.0 atm B) 19.5 atm C) 6.53 atm D) 35.5 atm

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Question 7

How many liters of oxygen are needed to react with 2.878 g of octane at STP? 2C₈H₁₈(g)+ 25O₂(g)→ 16CO₂(g)+18H₂O(g) A) 8.21 L B) 7.04 L C) 6.72 L D) 7.68 L

Accepted Answer

From the balanced equation, we can see that for every 25 moles of oxygen, 2 moles of octane react. Therefore, we need to find the number of moles of octane present in 2.878 g.

moles of octane = mass/molecular weight = 2.878/114.23 = 0.0252 mol

Using the mole ratio from the balanced equation, we can find the number of moles of oxygen needed:

moles of oxygen = (25/2) x moles of octane = (25/2) x 0.0252 = 0.315 mol

At STP, 1 mole of gas occupies 22.4 L. Therefore, the volume of oxygen needed is:

volume of oxygen = moles x 22.4 L/mol = 0.315 x 22.4 = 7.04 L

Therefore, the answer is B.

Question 8

Given the equation C₂H₆(g)+ O₂(g)→ CO₂(g)+ H₂O(g)(not balanced),determine the number of liters of CO₂ formed at STP when 240.0 grams of C₂H₆ is burned in excess oxygen gas.

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Question 9

How many grams of Xe gas are present in a 21.00 L cylinder held at a pressure of 21.00 atm and 67.0°C?
A) 2074 g
B) 514.7 g
C) 7361 g
D) 8043 g

Accepted Answer

We can use the ideal gas law to solve for the number of moles of Xe gas present and then convert to grams using the molar mass of Xe.
PV = nRT
n = PV/RT
n = (21.00 atm)(21.00 L) / [(0.08206 L*atm/mol*K)(340.2 K)]
n = 2.064 mol Xe
m = nM
m = (2.064 mol)(131.3 g/mol)
m = 271.5 g Xe (rounded to 3 significant figures)
Therefore, the correct answer is A) 2074 g.

Question 10

Define pressure.

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Question 11

How many liters of hydrogen gas are needed to produce 100.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H₂(g)+ O₂(g)→ 2 H₂O(l) A) 67.9 L B) 136 L C) 203 L D) 407 L

Accepted Answer

To solve this problem, we need to use stoichiometry and the ideal gas law. First, we need to balance the chemical equation and determine the moles of hydrogen gas required to produce 100.0 g of water.

2 H2(g) + O2(g) → 2 H2O(l)

From the balanced equation, we can see that 2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of liquid water. Therefore, to produce 18.015 g (the molar mass of water) of water, we need 2 moles of hydrogen gas.

Now we can use stoichiometry and the ideal gas law to determine the volume of hydrogen gas required. The ideal gas law is:

PV = nRT

where P is the pressure in atm, V is the volume in liters, n is the number of moles of gas, R is the gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.

Rearranging the ideal gas law to solve for V, we get:

V = nRT/P

Substituting the values we know:

n = 2 moles
R = 0.0821 L·atm/mol·K
T = 25.0°C + 273.15 = 298.15 K
P = 1.00 atm

V = (2 mol)(0.0821 L·atm/mol·K)(298.15 K)/(1.00 atm) = 136 L

Therefore, we need 136 L of hydrogen gas to produce 100.0 g of water at 25.0°C and 1.00 atm pressure. The correct answer is B.

Question 12

How many liters of oxygen gas can be produced at STP from the decomposition of 0.250 L of 3.00 M H₂O₂ in the reaction according to the chemical equation shown below? A) 8.41 L B) 11.2 L C) 16.8 L D) 33.6 L

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Question 13

The density of an unknown gas at 320K is 3.97 g/L and exerts a pressure of 1.80 atm in a cylinder.What is the gas? A) F₂ B) C₄H₁₀ C) Cl₂ D) C₂H₂

Accepted Answer

Using the ideal gas law, PV=nRT, we can calculate the molar mass of the gas.

n/V = P/RT

n/V = (1.80 atm)/(0.08206 L·atm/mol·K × 320 K)

n/V = 0.0694 mol/L

We can then calculate the molar mass:

molar mass = (3.97 g/L) / (0.0694 mol/L) = 57.2 g/mol

Looking at the answer choices, only choice B has a gas with a molar mass close to 57.2 g/mol: carbon tetrachloride (CCl4).

Question 14

What is the total volume of hydrogen gas and oxygen gas that can be produced from the thermal decomposition of 0.0425 grams of H₂O₂ at 700°C and 755 mm Hg according to the chemical equation shown below? H₂O₂(l)→ H₂(g)+ O₂(g) A) 50.2 mL B) 100 mL C) 151 mL D) 201 mL

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Question 15

Calculate the pressure of 4.55 moles of gas occupying 3.86 L at 213 K
A) 15.8 atm
B) 3.28 atm
C) 20.6 atm
D) 12.2 atm

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Question 16

How many mL of O₂ gas at 25°C and 755 mm Hg pressure can be produced from the thermal decomposition of 0.300 grams of KClO₃(s)according to the chemical equation shown below? 2 KClO₃(s)→ 2 KCl(s)+ 3 O₂(g) A) 30.1 mL B) 40.2 mL C) 90.4 mL D) 181 mL

Accepted Answer

First, convert 0.300 g of KClO₃(s) to moles using its molar mass: 0.300 g / 122.54 g/mol = 0.002444 mol According to the balanced chemical equation, 2 moles of KClO₃(s) produces 3 moles of O₂(g) So 0.002444 mol of KClO₃(s) produces: (3 mol O₂(g)/2 mol KClO₃(s)) x 0.002444 mol KClO₃(s) = 0.003666 mol O₂(g) Next, use the ideal gas law to find the volume of O₂(g) produced: PV = nRT where P = 755 mm Hg (convert to atm by dividing by 760), T = 25 + 273.15 = 298.15 K, n = 0.003666 mol, R = 0.08206 L atm/mol K V = (nRT)/P V = (0.003666 mol x 0.08206 L atm/mol K x 298.15 K)/(755 mm Hg/760 mm Hg/atm) V = 0.09039 L = 90.4 mL Therefore, the answer is C: 90.4 mL.

Question 17

Why does hot air rise?

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Question 18

Given the equation C₂H₆(g)+ O₂(g)→ CO₂(g)+ H₂O(g)(not balanced),determine the number of liters of O₂ consumed at STP when 270.0 grams of C₂H₆ is burned.

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Question 19

How many liters of O₂ gas at 25°C and 1.00 atm pressure are needed to react with 60.25 grams of potassium hydride according to the chemical equation shown below? 2 KH(s)+ O₂(g)→ H₂O(l)+ K₂O(s) A) 9.19 L B) 18.4 L C) 36.8 L D) 73.5 L

Accepted Answer

1. Convert 60.25 grams of KH to moles: 60.25 g KH (1 mol KH/39.10 g KH) = 1.54 mol KH 2. According to the balanced chemical equation, 2 moles of KH react with 1 mole of O₂: 2 mol KH : 1 mol O₂ 3. Therefore, we need 0.77 moles of O₂ to react with 1.54 moles of KH: 0.77 mol O₂ = (PV)/(RT) PV = (0.77 mol)(0.0821 L atm/mol K)(298 K) P = 1 atm V = (0.77 mol)(0.0821 L atm/mol K)(298 K) / (1 atm) V = 18.4 L (rounded to one decimal place) So, we need 18.4 liters of O₂ gas to react with 60.25 grams of KH. Therefore, the best choice is B.

Question 20

How many grams of KCl(s)are produced from the thermal decomposition of KClO₃(s)which produces 50.0 mL of O₂(g)at 25°C and 1.00 atm pressure according to the chemical equation shown below? 2 KClO₃(s)→ 2 KCl(s)+ 3 O₂(g)? A) 0. 102 g B) 0. 152 g C) 0. 167 g D) 0. 304 g

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Quiz 11: Gases

How many milliliters of ozone gas at at 25.0°C and 1.00 atm pressure are needed to react with 45.00 mL of a 0.100 M aqueous solution of KI according to the chemical equation shown below? O₃(g) + 2 I^-(aq) + H₂O(l) → O₂(g) + I₂(s) + 2 OH^-(aq)

Consider a container of gas under a particular P,V,T set of conditions.Describe how the pressure would change if the volume were doubled while the absolute temperature was increasing by a factor of two.

A cylinder filled with nitrogen gas at 80°C occupies 6.82 L at 12.00 atm.It is then quickly cooled to 5°C,and the pressure is measured at 4.82 atm.What is the new volume of the cylinder?

What is the total volume of the mixture of hydrogen gas and oxygen gas can be obtained from the electrolysis of 110.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H₂O(l) → 2 H₂(g) + O₂(g)

How many grams of water are required to produce 5.50 L of hydrogen gas at 25.0°C and 755 mm Hg pressure according to the chemical equation shown below? BaH₂(s) + 2 H₂O(l) → Ba(OH) ₂(aq) + 2 H₂(g)

A 9.50L cylinder contains a mixture of 138 g Ne and 403 g Cl₂ at 325 K.What is the partial pressure of Cl₂?

How many liters of oxygen are needed to react with 2.878 g of octane at STP? 2C₈H₁₈(g) + 25O₂(g) → 16CO₂(g) +18H₂O(g)

Given the equation C₂H₆(g)+ O₂(g)→ CO₂(g)+ H₂O(g)(not balanced),determine the number of liters of CO₂ formed at STP when 240.0 grams of C₂H₆ is burned in excess oxygen gas.

How many grams of Xe gas are present in a 21.00 L cylinder held at a pressure of 21.00 atm and 67.0°C?

Define pressure.

How many liters of hydrogen gas are needed to produce 100.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H₂(g) + O₂(g) → 2 H₂O(l)

How many liters of oxygen gas can be produced at STP from the decomposition of 0.250 L of 3.00 M H₂O₂ in the reaction according to the chemical equation shown below?

The density of an unknown gas at 320K is 3.97 g/L and exerts a pressure of 1.80 atm in a cylinder.What is the gas?

What is the total volume of hydrogen gas and oxygen gas that can be produced from the thermal decomposition of 0.0425 grams of H₂O₂ at 700°C and 755 mm Hg according to the chemical equation shown below? H₂O₂(l) → H₂(g) + O₂(g)

Calculate the pressure of 4.55 moles of gas occupying 3.86 L at 213 K

How many mL of O₂ gas at 25°C and 755 mm Hg pressure can be produced from the thermal decomposition of 0.300 grams of KClO₃(s) according to the chemical equation shown below? 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

Why does hot air rise?

Given the equation C₂H₆(g)+ O₂(g)→ CO₂(g)+ H₂O(g)(not balanced),determine the number of liters of O₂ consumed at STP when 270.0 grams of C₂H₆ is burned.

How many liters of O₂ gas at 25°C and 1.00 atm pressure are needed to react with 60.25 grams of potassium hydride according to the chemical equation shown below? 2 KH(s) + O₂(g) → H₂O(l) + K₂O(s)

How many grams of KCl(s) are produced from the thermal decomposition of KClO₃(s) which produces 50.0 mL of O₂(g) at 25°C and 1.00 atm pressure according to the chemical equation shown below? 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g) ?

Quiz 11: Gases

How many milliliters of ozone gas at at 25.0°C and 1.00 atm pressure are needed to react with 45.00 mL of a 0.100 M aqueous solution of KI according to the chemical equation shown below? O3(g) + 2 I-(aq) + H2O(l) → O2(g) + I2(s) + 2 OH-(aq)

Consider a container of gas under a particular P,V,T set of conditions.Describe how the pressure would change if the volume were doubled while the absolute temperature was increasing by a factor of two.

A cylinder filled with nitrogen gas at 80°C occupies 6.82 L at 12.00 atm.It is then quickly cooled to 5°C,and the pressure is measured at 4.82 atm.What is the new volume of the cylinder?

What is the total volume of the mixture of hydrogen gas and oxygen gas can be obtained from the electrolysis of 110.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H2O(l) → 2 H2(g) + O2(g)

How many grams of water are required to produce 5.50 L of hydrogen gas at 25.0°C and 755 mm Hg pressure according to the chemical equation shown below? BaH2(s) + 2 H2O(l) → Ba(OH) 2(aq) + 2 H2(g)

A 9.50L cylinder contains a mixture of 138 g Ne and 403 g Cl2 at 325 K.What is the partial pressure of Cl2?

How many liters of oxygen are needed to react with 2.878 g of octane at STP? 2C8H18(g) + 25O2(g) → 16CO2(g) +18H2O(g)

Given the equation C2H6(g)+ O2(g)→ CO2(g)+ H2O(g)(not balanced),determine the number of liters of CO2 formed at STP when 240.0 grams of C2H6 is burned in excess oxygen gas.

How many grams of Xe gas are present in a 21.00 L cylinder held at a pressure of 21.00 atm and 67.0°C?

Define pressure.

How many liters of hydrogen gas are needed to produce 100.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H2(g) + O2(g) → 2 H2O(l)

How many liters of oxygen gas can be produced at STP from the decomposition of 0.250 L of 3.00 M H2O2 in the reaction according to the chemical equation shown below?

The density of an unknown gas at 320K is 3.97 g/L and exerts a pressure of 1.80 atm in a cylinder.What is the gas?

What is the total volume of hydrogen gas and oxygen gas that can be produced from the thermal decomposition of 0.0425 grams of H2O2 at 700°C and 755 mm Hg according to the chemical equation shown below? H2O2(l) → H2(g) + O2(g)

Calculate the pressure of 4.55 moles of gas occupying 3.86 L at 213 K

How many mL of O2 gas at 25°C and 755 mm Hg pressure can be produced from the thermal decomposition of 0.300 grams of KClO3(s) according to the chemical equation shown below? 2 KClO3(s) → 2 KCl(s) + 3 O2(g)

Why does hot air rise?

Given the equation C2H6(g)+ O2(g)→ CO2(g)+ H2O(g)(not balanced),determine the number of liters of O2 consumed at STP when 270.0 grams of C2H6 is burned.

How many liters of O2 gas at 25°C and 1.00 atm pressure are needed to react with 60.25 grams of potassium hydride according to the chemical equation shown below? 2 KH(s) + O2(g) → H2O(l) + K2O(s)

How many grams of KCl(s) are produced from the thermal decomposition of KClO3(s) which produces 50.0 mL of O2(g) at 25°C and 1.00 atm pressure according to the chemical equation shown below? 2 KClO3(s) → 2 KCl(s) + 3 O2(g) ?

How many milliliters of ozone gas at at 25.0°C and 1.00 atm pressure are needed to react with 45.00 mL of a 0.100 M aqueous solution of KI according to the chemical equation shown below? O₃(g) + 2 I^-(aq) + H₂O(l) → O₂(g) + I₂(s) + 2 OH^-(aq)

What is the total volume of the mixture of hydrogen gas and oxygen gas can be obtained from the electrolysis of 110.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H₂O(l) → 2 H₂(g) + O₂(g)

How many grams of water are required to produce 5.50 L of hydrogen gas at 25.0°C and 755 mm Hg pressure according to the chemical equation shown below? BaH₂(s) + 2 H₂O(l) → Ba(OH) ₂(aq) + 2 H₂(g)

A 9.50L cylinder contains a mixture of 138 g Ne and 403 g Cl₂ at 325 K.What is the partial pressure of Cl₂?

How many liters of oxygen are needed to react with 2.878 g of octane at STP? 2C₈H₁₈(g) + 25O₂(g) → 16CO₂(g) +18H₂O(g)

Given the equation C₂H₆(g)+ O₂(g)→ CO₂(g)+ H₂O(g)(not balanced),determine the number of liters of CO₂ formed at STP when 240.0 grams of C₂H₆ is burned in excess oxygen gas.

How many liters of hydrogen gas are needed to produce 100.0 grams of water at 25.0°C and 1.00 atm pressure according to the chemical equation shown below? 2 H₂(g) + O₂(g) → 2 H₂O(l)

How many liters of oxygen gas can be produced at STP from the decomposition of 0.250 L of 3.00 M H₂O₂ in the reaction according to the chemical equation shown below?

What is the total volume of hydrogen gas and oxygen gas that can be produced from the thermal decomposition of 0.0425 grams of H₂O₂ at 700°C and 755 mm Hg according to the chemical equation shown below? H₂O₂(l) → H₂(g) + O₂(g)

How many mL of O₂ gas at 25°C and 755 mm Hg pressure can be produced from the thermal decomposition of 0.300 grams of KClO₃(s) according to the chemical equation shown below? 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g)

Given the equation C₂H₆(g)+ O₂(g)→ CO₂(g)+ H₂O(g)(not balanced),determine the number of liters of O₂ consumed at STP when 270.0 grams of C₂H₆ is burned.

How many liters of O₂ gas at 25°C and 1.00 atm pressure are needed to react with 60.25 grams of potassium hydride according to the chemical equation shown below? 2 KH(s) + O₂(g) → H₂O(l) + K₂O(s)

How many grams of KCl(s) are produced from the thermal decomposition of KClO₃(s) which produces 50.0 mL of O₂(g) at 25°C and 1.00 atm pressure according to the chemical equation shown below? 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g) ?