In the reaction of 500 g of sulfur dioxide (SO,) with excess oxygen, what volume of sulfur trioxide (So be produced at STP?

• 1121

• 16.81

• 22:21

• 33.6 L

Given the decomposition of 0.500 moles of potassium chlorate (KCIO,), calculate the volume of oxygen (0) gas produced at STP.

• 11.21

• 16.8 L

• 22.4 L

• 33.6 L

During an automotive airbag deployment, sodium azide (NaN,) decomposes rapidly to produce nitrogen gas (N₂). For safety reasons, an engineer calculates the amount of gas produced. If 0.1 moles of sodium azide (NaN) decompose completely, how many liters of nitrogen gas will be produced at STP?

• 1.211

• 2.24 L

• 5.60 L

• 22.4 L

A chemical plant produces sulfur dioxide (SO₂) by burning sulfur in the presence of oxygen. The gas is then measured for environmental monitoring. If 100 g of sulfur (S) is burned, how many liters of sulfur dioxide (SO₂) gas will be produced at STP?

• 44.8 L

• 224 L

• 11.2 L

• 89.6 L

In a classroom demonstration, 5 grams of magnesium reacts with hydrochloric acid to produce hydrogen gas (H₂) What volume of hydrogen gas is produced at 25°C and 1 atm if 5 grams of magnesium reacts completely?

• 2.01

• 35 L

• 4.5 L

• 5.0 L

You are tasked with designing an experiment where a known mass of calcium carbonate (CaCO,) reacts with hydrochloric acid to produce carbon dioxide (CO₂). How many liters of carbon dioxide gas will be produced at STP if 10 g of calcium carbonate reacts completely?

• 1.12 L

• 2.24 L

• 4.48 L

• 5.60 L

A combustion reaction of propane (C,H.) occurs in a lab. The reaction proceeds completely, and you are asked to determine the amount of water vapor produced If 1.5 moles of propane are burned with excess oxygen, how many moles of water vapor are produced?

• 1.5 moles

• 2.0 moles

• 3.0 moles

• 4.5 moles

A student observes that two different gases are stored at the same temperature but have different rates of diffusion. Based on kinetic molecular theory, how can the different diffusion rates of gases be explained?

• The gases have different volumes.

• The temperature of both gases is different.

• The masses of the gas particles differ.

• The gases have attractive forces between them.

A scientist measures the pressure of a gas and finds that increasing the volume of the container decreases the pressure. Using the kinetic molecular theory, what is the reason for this decrease in pressure?

• The gas particles move faster in a larger container.

• The gas particles stop moving in a larger container.

• The volume of the gas particles increases with the container.

• The gas particles have more space to move, so they collide less often with the walls.

A researcher lowers the temperature of a gas and observes a decrease in the kinetic energy of the gas particles. How does kinetic molecular theory explain the relationship between temperature and the behavior of gas particles?

• Lower temperature decreases the mass of the gas particles.

• Lower temperature increases the volume of the gas particles.

• Lower temperature causes the gas particles to attract each other.

• Lower temperature reduces the speed and energy of the gas particles.