91Ó°ÊÓ

How many moles of helium gas (He) would be required to fill a \(22-\) L container at a temperature of \(35^{\circ} \mathrm{C}\) and a pressure of 3.1 atm?

Before a reaction, two gases share a container at a temperature of 200 \(\mathrm{K}\) . After the reaction, the product is in the same container at a temperature of 400 \(\mathrm{K} .\) If both \(V\) and \(P\) are constant, what must be true of \(n\) ?

Why must an equation be balanced before using it to determine the volumes of gases involved in a reaction?

It is not necessary to consider temperature and pressure when using a balanced equation to determine relative gas volume. Why?

What information do you need to solve a volume-mass problem that involves gases?

Explain why the coefficients in a balanced chemical equation represent not only molar amounts but also relative volumes for gases.

Do the coefficients in a balanced chemical equation represent volume ratios for solids and liquids? Explain.

A 6.5 -L sample of hydrogen sulfide is treated with a catalyst to promote the reaction shown below. $$2 \mathrm{H}_{2} \mathrm{S}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+2 \mathrm{S}(\mathrm{s})$$ If the \(\mathrm{H}_{2} \mathrm{S}\) reacts completely at 2.0 atm and \(290 \mathrm{K},\) how much water vapor, in grams, is produced?

Use the reaction shown below to answer these questions. $$2 \mathrm{CO}(\mathrm{g})+2 \mathrm{NO}(\mathrm{g}) \rightarrow \mathrm{N}_{2}(\mathrm{g})+2 \mathrm{CO}_{2}(\mathrm{g})$$ a. What is the volume ratio of carbon monoxide to carbon dioxide in the balanced equation? b. If 42.7 g of CO is reacted completely at STP, what volume of \(\mathrm{N}_{2}\) gas will be produced?

When 3.00 L of propane gas is completely combusted to form water vapor and carbon dioxide at \(350^{\circ} \mathrm{C}\) and 0.990 atm, what mass of water vapor results?