Mole Ratios and Gas Laws

This video tutorial by Mrs. E covers the connection between the ideal gas law and stoichiometry. It explains how to use mole ratios from balanced chemical equations and the ideal gas law (PV=nRT) to solve various chemistry problems. The tutorial includes examples such as calculating the grams of zinc needed to produce hydrogen gas, finding moles of carbon dioxide, determining sodium azide for nitrogen gas production, and calculating the volume of H2S required to produce sulfur.

What is the primary relationship between the coefficients in a balanced chemical equation?

• They show the mole ratios between reactants and products.

• They determine the speed of the reaction.

• They indicate the volume ratios of gases involved.

• They represent the mass ratios of reactants and products.

Which variable in the ideal gas law is used to find the number of moles of a gas?

• Pressure (P)

• Volume (V)

• Temperature (T)

• Moles (n)

How many liters of any gas at STP is equivalent to one mole?

• 18.0 liters

• 20.0 liters

• 24.0 liters

• 22.4 liters

In the problem involving zinc and hydrogen gas, what is the calculated mass of zinc required?

• 5.0 grams

• 7.0 grams

• 12.0 grams

• 10.0 grams

When not at STP, which method is used to find the moles of a gas?

• Using temperature conversion

• Using mass ratios

• Using PV=nRT

• Using molar volume

What is the mole ratio between carbon dioxide and calcium carbonate in the given problem?

• 2:1

• 1:2

• 3:1

• 1:1

In the nitrogen gas problem, what is the mole ratio between nitrogen and sodium nitrite?

• 1:1

• 2:3

• 1:2

• 3:2

What is the molar mass of sulfur used in the final problem?

• 32.066 g/mol

• 28.085 g/mol

• 35.453 g/mol

• 30.974 g/mol

How many moles of H2S are needed to produce 65 grams of sulfur?

• 1.351 moles

• 1.500 moles

• 1.200 moles

• 1.000 moles

What is the calculated volume of H2S required in the final problem?

• 40.0 liters

• 36.3 liters

• 30.0 liters

• 45.0 liters