Question

part d find the number of moles of water that can be formed if you have 174 mol of hydrogen gas and 82 mol of oxygen gas. express your answer with the appropriate units. view available hint(s)

Explanation:

Step1: Write the chemical reaction

The reaction for the formation of water from hydrogen and oxygen is $2H_2 + O_2
ightarrow2H_2O$.

Step2: Determine the limiting reactant

The mole - ratio of $H_2$ to $O_2$ in the reaction is 2:1. Given $n_{H_2}=174\ mol$ and $n_{O_2} = 82\ mol$. For $82\ mol$ of $O_2$, the amount of $H_2$ required is $2\times82=164\ mol$. Since $174\ mol$ of $H_2$ is available, $O_2$ is the limiting reactant.

Step3: Calculate moles of water

From the mole - ratio of $O_2$ to $H_2O$ (1:2), if $n_{O_2}=82\ mol$, then $n_{H_2O}=2\times n_{O_2}$. So $n_{H_2O}=2\times82 = 164\ mol$.

Answer:

164 mol