Questions: Water forms when hydrogen gas reacts explosively with oxygen gas according to the balanced equation: O2(g) + ... H2(g) -> ... H2O(g) How many mol of H2O result from the complete reaction of 24.6 mol O2? Assume that there is more than enough H2. 6.15 mol 24.6 mol 49.2 mol 12.3 mol

Solution Steps

The balanced chemical equation for the reaction between hydrogen gas (\(\mathrm{H}_2\)) and oxygen gas (\(\mathrm{O}_2\)) to form water (\(\mathrm{H}_2\mathrm{O}\)) is: \[ 2\mathrm{H}_2(\mathrm{~g}) + \mathrm{O}_2(\mathrm{~g}) \longrightarrow 2\mathrm{H}_2\mathrm{O}(\mathrm{~g}) \]

From the balanced equation, we see that 1 mole of \(\mathrm{O}_2\) reacts with 2 moles of \(\mathrm{H}_2\) to produce 2 moles of \(\mathrm{H}_2\mathrm{O}\). Therefore, the mole ratio of \(\mathrm{O}_2\) to \(\mathrm{H}_2\mathrm{O}\) is 1:2.

Given that we have 24.6 moles of \(\mathrm{O}_2\), we can use the mole ratio to find the moles of \(\mathrm{H}_2\mathrm{O}\) produced: \[ \text{Moles of } \mathrm{H}_2\mathrm{O} = 24.6 \, \text{mol} \, \mathrm{O}_2 \times \frac{2 \, \text{mol} \, \mathrm{H}_2\mathrm{O}}{1 \, \text{mol} \, \mathrm{O}_2} = 49.2 \, \text{mol} \, \mathrm{H}_2\mathrm{O} \]

Final Answer