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Problem 79

Metal hydrides react with water to form hydrogen gas and the metal hydroxide. For example, $$ \mathrm{SrH}_{2}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Sr}(\mathrm{OH})_{2}(s)+2 \mathrm{H}_{2}(g) $$ You wish to calculate the mass (g) of hydrogen gas that can be prepared from 5.70 $\mathrm{g}$ of $\mathrm{SrH}_{2}$ and 4.75 $\mathrm{g}$ of $\mathrm{H}_{2} \mathrm{O}$ . (a) What amount (mol) of $\mathrm{H}_{2}$ can be produced from the given mass of $\mathrm{SrH}_{2} ?$ (b) What amount (mol) of $\mathrm{H}_{2}$ can be produced from the given mass of $\mathrm{H}_{2} \mathrm{O}$ ? (c) Which is the limiting reactant? (d) How many grams of $\mathrm{H}_{2}$ can be produced?

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## Recommended Questions

How many liters of hydrogen gas can be

produced at 300.0 $\mathrm{K}$ and 104 $\mathrm{kPa}$ if 20.0 $\mathrm{g}$

of sodium metal is reacted with water

according to the following equation?

$$2 \mathrm{Na}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow 2 \mathrm{NaOH}(a q)+\mathrm{H}_{2}(g)$$

Hydrogen sulfide is an impurity in natural gas that must be removed. One common removal method is called the Claus process, which relies on the reaction:

$$

8 \mathrm{H}_{2} \mathrm{S}(g)+4 \mathrm{O}_{2}(g) \longrightarrow \mathrm{S}_{8}(l)+8 \mathrm{H}_{2} \mathrm{O}(g)

$$

Under optimal conditions the Claus process gives 98$\%$ yield of $S_{8}$ from $\mathrm{H}_{2}$ . If you started with 30.0 g of $\mathrm{H}_{2} \mathrm{S}$ and 50.0 $\mathrm{g}$ of $\mathrm{O}_{2},$ how many grams of $\mathrm{S}_{8}$ would be produced, assuming 98$\%$ yield?

Sodium hydroxide reacts with carbon dioxide as follows:

$$

2 \mathrm{NaOH}(s)+\mathrm{CO}_{2}(g) \longrightarrow \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l)

$$

Which is the limiting reactant when 1.85 mol $\mathrm{NaOH}$ and 1.00 $\mathrm{mol} \mathrm{CO}_{2}$ are allowed to react? How many moles of $\mathrm{Na}_{2} \mathrm{CO}_{3}$ can be produced? How many moles of the excess reactant remain after the completion of the reaction?