Problem 30
How many milliliters of carbon dioxide gas at STP are produced from the decomposition of \(5.00 \mathrm{~g}\) of iron(III) carbonate? $$\mathrm{Fe}_{2}\left(\mathrm{CO}_{3}\right)_{3}(s) \longrightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3\mathrm{CO}_{2}(g)$$
Problem 31
How many milliliters of oxygen gas at STP are released from heating \(5.00 \mathrm{~g}\) of calcium chlorate? $$\mathrm{Ca}\left(\mathrm{ClO}_{3}\right)_{2}(s) \longrightarrow \mathrm{CaCl}_{2}(\mathrm{~s})+3\mathrm{O}_{2}(g)$$
Problem 32
How many milliliters of oxygen gas at STP are released from heating \(2.50 \mathrm{~g}\) of mercuric oxide? $$2 \mathrm{HgO}(s) \longrightarrow 2 \mathrm{Hg}(l)+\mathrm{O}_{2}(g)$$
Problem 33
What mass of magnesium metal reacts with sulfuric acid to produce \(225 \mathrm{~mL}\) of hydrogen gas at STP? $$\mathrm{Mg}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{MgSO}_{4}(aq)+\mathrm{H}_{2}(g)$$
Problem 35
How many grams of sodium metal react with water to give \(75.0 \mathrm{~mL}\) of hydrogen gas at STP? $$\mathrm{Na}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{NaOH}(a +\mathrm{H}_{2}(g)$$
Problem 36
How many grams of hydrogen peroxide must decompose to give \(55.0 \mathrm{~mL}\) of oxygen gas at STP? $$\mathrm{H}_{2} \mathrm{O}_{2}(l) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)$$
Problem 37
Assuming all gases are at the same temperature and pressure, how many milliliters of iodine vapor react with \(125 \mathrm{~mL}\) of hydrogen gas? $$\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \longrightarrow 2 \mathrm{HI}(g)$$
Problem 39
Assuming all gases are at the same temperature and pressure, how many milliliters of nitrogen gas react to give \(45.0 \mathrm{~mL}\) of ammonia gas? $$3 \mathrm{H}_{2}(g)+\mathrm{N}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)$$
Problem 41
Assuming all gases are at the same temperature and pressure, how many liters of oxygen gas react with \(10.0 \mathrm{~L}\) of carbon monoxide? $$2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)$$
Problem 49
If 1.00 mol of nitrogen monoxide gas and 1.00 mol of oxygen gas react, what is the limiting reactant and how many moles of \(\mathrm{NO}_{2}\) are produced from the reaction? $$2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)$$
