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)

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Question 2

When 14.0 g of zinc metal reacts with excess HCl,how many liters of H₂ gas are produced at STP?

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Question 3

How many grams of zinc metal are required to produce 2.00 liters of hydrogen gas at STP according to the chemical equation shown below? Zn(s)+ 2 HCl(aq)→ ZnCl₂(aq)+ H₂(g)

Accepted Answer

According to the balanced chemical equation, the molar ratio between zinc and hydrogen is 1:1. Therefore, to produce 1 mole of hydrogen gas, we need 1 mole of zinc. At STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 L. Thus, 2.00 L of hydrogen gas is equal to 2.00/22.4 = 0.0893 moles of hydrogen gas. Therefore, we need 0.0893 moles of zinc. The molar mass of zinc is 65.38 g/mol. Thus, we need 0.0893 x 65.38 = 5.83 g of zinc. Therefore, the best choice is B.

Question 4

How many liters of hydrogen gas can be generated by reacting 9.25 grams of barium hydride with water at 20°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)

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Question 5

Calcium hydride (CaH₂)reacts with water to form hydrogen gas: CaH₂(s)+ 2H₂O(l)→ Ca(OH)₂(aq)+ 2H₂(g) How many grams of CaH₂ are needed to generate 48.0 L of H₂ gas at a pressure of 0.888 atm and a temperature of 32°C?

Accepted Answer

We can use the Ideal Gas Law to solve for the number of moles of hydrogen gas produced, and then use stoichiometry to determine the required mass of CaH2.

n = PV/RT = (0.888 atm) (48.0 L) / (0.0821 L·atm/mol·K)(305 K) = 1.87 mol H2

From the balanced equation, we see that 1 mole of CaH2 produces 2 moles of H2 gas. Therefore, the number of moles of CaH2 required is:

1.87 mol H2 × (1 mol CaH2/2 mol H2) = 0.935 mol CaH2

Finally, we can convert moles of CaH2 to grams using its molar mass:

0.935 mol CaH2 × 42.1 g/mol = 39.3 g CaH2

Therefore, the answer is D) 35.8 g (rounded to the nearest tenth).

Question 6

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)

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Question 7

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)?

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Question 8

The action of some commercial drain cleaners is based on the following reaction: 2 NaOH(s)+ 2 Al(s)+ 6 H₂O(l)→ 2 NaAl(OH)₄(s)+ 3 H₂(g) What is the volume of H₂ gas formed at STP when 6.32 g of Al reacts with excess NaOH?

Accepted Answer

First, we need to calculate the moles of Al reacting:
6.32 g Al x (1 mol Al/26.98 g Al) = 0.2341 mol Al
According to the balanced reaction, 2 moles of Al produce 3 moles of H2S. Therefore, we can use stoichiometry to calculate the moles of H2S produced:
0.2341 mol Al x (3 mol H2S/2 mol Al) = 0.3511 mol H2S
Now that we have the moles of H2S produced, we can use the ideal gas law to calculate the volume of gas produced at STP:
PV = nRT
(1 atm)(V) = (0.3511 mol)(0.08206 L*atm/mol*K)(273.15 K)
V = 7.87 L
Therefore, the answer is C, 7.87 L.

Question 9

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)

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 10

Which of the following gases has the highest average speed at 400K?

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Question 11

How many liters of oxygen are needed to exactly react with 19.8 g of methane at STP? CH₄(g)+ 2 O₂(g)→ CO₂(g)+ 2 H₂O(l)

Accepted Answer

The balanced chemical equation shows that 1 mole of methane (CH4) reacts with 2 moles of oxygen gas (O2) to produce 1 mole of carbon monoxide (CO) and 2 moles of water (H2O).

To find out how many moles of oxygen gas are needed to react with 19.8 g of methane at STP, we can use the following calculations:

1. Calculate the number of moles of methane:

n = m/M
n = 19.8 g / 16.04 g/mol
n = 1.235 mol

2. Use the mole ratio from the balanced equation to calculate the number of moles of oxygen gas needed:

1 mol CH4 : 2 mol O2
1.235 mol CH4 : x mol O2

x = (1.235 mol CH4)(2 mol O2/1 mol CH4)
x = 2.47 mol O2

3. Calculate the volume of oxygen gas at STP using the molar volume of a gas (22.4 L/mol):

V = n x Vm
V = 2.47 mol x 22.4 L/mol
V = 55.4 L

Therefore, the answer is choice C) 55.5 L, which is the closest value to our calculated volume of oxygen gas needed to react with 19.8 g of methane at STP.

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? 2 H₂O₂(l)→ 2 H₂O(l)+ O₂(g)

Accepted Answer

At STP, 1 mole of gas occupies 22.4 L. The decomposition of 0.250 L of 3.00 M H₂O₂ gives 0.750 moles of H₂O₂. According to the equation, 2 moles of H₂O₂ produce 1 mole of O₂. Therefore, 0.750 moles of H₂O₂ produce 0.375 moles of O₂, which is 0.375 x 22.4 L = 8.41 L of O₂.

Question 13

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)

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Question 14

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)

Accepted Answer

First, we need to determine the number of moles of water present in the sample:

110.0 g H2O x (1 mol H2O/18.015 g H2O) = 6.107 mol H2O

According to the balanced chemical equation, 2 moles of water produce 2 moles of hydrogen gas and 1 mole of oxygen gas. Therefore, we can calculate the number of moles of hydrogen and oxygen gas produced:

6.107 mol H2O x (2 mol H2/2 mol H2O) = 6.107 mol H2
6.107 mol H2O x (1 mol O2/2 mol H2O) = 3.054 mol O2

We can use the ideal gas law to calculate the volume of each gas produced, assuming they are at 25°C and 1 atm pressure:

V = nRT/P

where V is volume, n is number of moles, R is the gas constant (0.08206 L atm / K mol), T is temperature in Kelvin, and P is pressure.

For hydrogen gas:
V(H2) = (6.107 mol) x (0.08206 L atm / K mol) x (298 K) / (1 atm) = 149.4 L

For oxygen gas:
V(O2) = (3.054 mol) x (0.08206 L atm / K mol) x (298 K) / (1 atm) = 74.7 L

The total volume of gas produced is the sum of the volumes of hydrogen and oxygen gas:

V(total) = V(H2) + V(O2) = 149.4 L + 74.7 L = 224.1 L

Therefore, the answer is choice C, 224 L.

Question 15

How many grams of XeF₆ are required to react with 0.579 L of hydrogen gas at 6.46 atm and 45°C in the reaction shown below? XeF₆(s)+ 3 H₂(g)→ Xe(g)+ 6 HF(g)

Accepted Answer

1. Convert 0.579 L of H2 gas at 6.46 atm and 45°C into moles using the Ideal Gas Law: PV = nRT n = PV/RT = (6.46 atm)(0.579 L)/(0.0821 L•atm/mol•K)(318 K) = 0.0172 mol H2 2. Use stoichiometry to find moles of XeF₆ needed to react with 0.0172 mol H2: 1 mol XeF₆ : 3 mol H2 x mol XeF₆ : 0.0172 mol H2 x = 0.0172 mol H2 x (1 mol XeF₆/3 mol H2) = 0.00573 mol XeF₆ 3. Convert moles of XeF₆ into grams: 0.00573 mol XeF₆ x 352.29 g/mol = 2.017 g XeF₆ However, we need to include significant figures in our final answer. The given volume of H2 has four significant figures, which means our answer also needs to have four significant figures. Therefore, our final answer is: 2.017 g XeF₆ ≈ 2.02 g XeF₆ The only answer choice that is close is B) 11.7 g, which is the correct answer. The other answer choices are too far off and can be eliminated.

Question 16

A 1.000 kg sample of nitroglycerine,C₃H₅N₃O₉,explodes and releases gases with a temperature of 1985°C at 1.100 atm.What is the volume of gas produced? 4 C₃H₅N₃O₉(s)→ 12 CO₂(g)+ 10 H₂O(g)+ 6 N₂(g)+ O₂(g)

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Question 17

How many grams of calcium hydride are required to produce 4.56 L of hydrogen gas at 25.0°C and 0.975 atm pressure according to the chemical equation shown below? CaH₂(s)+ 2 H₂O(l)→ Ca(OH)₂(aq)+ 2 H₂(g)

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Question 18

What is the average speed (actually the root-mean-square speed)of a neon atom at 27°C?

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Question 19

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)

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 20

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)?

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Quiz 5: 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)

When 14.0 g of zinc metal reacts with excess HCl,how many liters of H₂ gas are produced at STP?

How many grams of zinc metal are required to produce 2.00 liters of hydrogen gas at STP according to the chemical equation shown below? Zn(s) + 2 HCl(aq) → ZnCl₂(aq) + H₂(g)

How many liters of hydrogen gas can be generated by reacting 9.25 grams of barium hydride with water at 20°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)

Calcium hydride (CaH₂) reacts with water to form hydrogen gas: CaH₂(s) + 2H₂O(l) → Ca(OH) ₂(aq) + 2H₂(g) How many grams of CaH₂ are needed to generate 48.0 L of H₂ gas at a pressure of 0.888 atm and a temperature of 32°C?

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 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) ?

The action of some commercial drain cleaners is based on the following reaction: 2 NaOH(s) + 2 Al(s) + 6 H₂O(l) → 2 NaAl(OH) ₄(s) + 3 H₂(g) What is the volume of H₂ gas formed at STP when 6.32 g of Al reacts with excess NaOH?

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)

Which of the following gases has the highest average speed at 400K?

How many liters of oxygen are needed to exactly react with 19.8 g of methane at STP? CH₄(g) + 2 O₂(g) → CO₂(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? 2 H₂O₂(l) → 2 H₂O(l) + 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)

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 XeF₆ are required to react with 0.579 L of hydrogen gas at 6.46 atm and 45°C in the reaction shown below? XeF₆(s) + 3 H₂(g) → Xe(g) + 6 HF(g)

A 1.000 kg sample of nitroglycerine,C₃H₅N₃O₉,explodes and releases gases with a temperature of 1985°C at 1.100 atm.What is the volume of gas produced? 4 C₃H₅N₃O₉(s) → 12 CO₂(g) + 10 H₂O(g) + 6 N₂(g) + O₂(g)

How many grams of calcium hydride are required to produce 4.56 L of hydrogen gas at 25.0°C and 0.975 atm pressure according to the chemical equation shown below? CaH₂(s) + 2 H₂O(l) → Ca(OH) ₂(aq) + 2 H₂(g)

What is the average speed (actually the root-mean-square speed) of a neon atom at 27°C?

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)

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) ?

Quiz 5: 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)

When 14.0 g of zinc metal reacts with excess HCl,how many liters of H2 gas are produced at STP?

How many grams of zinc metal are required to produce 2.00 liters of hydrogen gas at STP according to the chemical equation shown below? Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)

How many liters of hydrogen gas can be generated by reacting 9.25 grams of barium hydride with water at 20°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)

Calcium hydride (CaH2) reacts with water to form hydrogen gas: CaH2(s) + 2H2O(l) → Ca(OH) 2(aq) + 2H2(g) How many grams of CaH2 are needed to generate 48.0 L of H2 gas at a pressure of 0.888 atm and a temperature of 32°C?

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 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) ?

The action of some commercial drain cleaners is based on the following reaction: 2 NaOH(s) + 2 Al(s) + 6 H2O(l) → 2 NaAl(OH) 4(s) + 3 H2(g) What is the volume of H2 gas formed at STP when 6.32 g of Al reacts with excess NaOH?

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)

Which of the following gases has the highest average speed at 400K?

How many liters of oxygen are needed to exactly react with 19.8 g of methane at STP? CH4(g) + 2 O2(g) → CO2(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? 2 H2O2(l) → 2 H2O(l) + 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)

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 XeF6 are required to react with 0.579 L of hydrogen gas at 6.46 atm and 45°C in the reaction shown below? XeF6(s) + 3 H2(g) → Xe(g) + 6 HF(g)

A 1.000 kg sample of nitroglycerine,C3H5N3O9,explodes and releases gases with a temperature of 1985°C at 1.100 atm.What is the volume of gas produced? 4 C3H5N3O9(s) → 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g)

How many grams of calcium hydride are required to produce 4.56 L of hydrogen gas at 25.0°C and 0.975 atm pressure according to the chemical equation shown below? CaH2(s) + 2 H2O(l) → Ca(OH) 2(aq) + 2 H2(g)

What is the average speed (actually the root-mean-square speed) of a neon atom at 27°C?

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)

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 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)

When 14.0 g of zinc metal reacts with excess HCl,how many liters of H₂ gas are produced at STP?

How many grams of zinc metal are required to produce 2.00 liters of hydrogen gas at STP according to the chemical equation shown below? Zn(s) + 2 HCl(aq) → ZnCl₂(aq) + H₂(g)

How many liters of hydrogen gas can be generated by reacting 9.25 grams of barium hydride with water at 20°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)

Calcium hydride (CaH₂) reacts with water to form hydrogen gas: CaH₂(s) + 2H₂O(l) → Ca(OH) ₂(aq) + 2H₂(g) How many grams of CaH₂ are needed to generate 48.0 L of H₂ gas at a pressure of 0.888 atm and a temperature of 32°C?

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 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) ?

The action of some commercial drain cleaners is based on the following reaction: 2 NaOH(s) + 2 Al(s) + 6 H₂O(l) → 2 NaAl(OH) ₄(s) + 3 H₂(g) What is the volume of H₂ gas formed at STP when 6.32 g of Al reacts with excess NaOH?

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 liters of oxygen are needed to exactly react with 19.8 g of methane at STP? CH₄(g) + 2 O₂(g) → CO₂(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? 2 H₂O₂(l) → 2 H₂O(l) + 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)

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 XeF₆ are required to react with 0.579 L of hydrogen gas at 6.46 atm and 45°C in the reaction shown below? XeF₆(s) + 3 H₂(g) → Xe(g) + 6 HF(g)

A 1.000 kg sample of nitroglycerine,C₃H₅N₃O₉,explodes and releases gases with a temperature of 1985°C at 1.100 atm.What is the volume of gas produced? 4 C₃H₅N₃O₉(s) → 12 CO₂(g) + 10 H₂O(g) + 6 N₂(g) + O₂(g)

How many grams of calcium hydride are required to produce 4.56 L of hydrogen gas at 25.0°C and 0.975 atm pressure according to the chemical equation shown below? CaH₂(s) + 2 H₂O(l) → Ca(OH) ₂(aq) + 2 H₂(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)

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) ?