the balanced chemical equation for the reaction of hydrogen and oxygen is shown below.\n2h₂ + o₂ → 2h₂o\nthe…

the balanced chemical equation for the reaction of hydrogen and oxygen is shown below.\n2h₂ + o₂ → 2h₂o\nthe number of moles of hydrogen that is needed to produce 0.253 mol of water is\no smaller than 0.253 mol.\no much greater than 0.253 mol.\no slightly greater than 0.253 mol.\no equal to 0.253 mol.

the balanced chemical equation for the reaction of hydrogen and oxygen is shown below.\n2h₂ + o₂ → 2h₂o\nthe number of moles of hydrogen that is needed to produce 0.253 mol of water is\no smaller than 0.253 mol.\no much greater than 0.253 mol.\no slightly greater than 0.253 mol.\no equal to 0.253 mol.

Answer

Explanation:

Step1: Analyze mole - ratio from equation

From the balanced equation $2H_2 + O_2\rightarrow2H_2O$, the mole - ratio of $H_2$ to $H_2O$ is $2:2$ or $1:1$.

Step2: Calculate moles of hydrogen

If the mole - ratio of $H_2$ to $H_2O$ is $1:1$, and we want to produce $n_{H_2O}=0.253$ mol of water, then the moles of hydrogen needed $n_{H_2}$ is calculated as follows: Since $\frac{n_{H_2}}{n_{H_2O}} = 1$, $n_{H_2}=n_{H_2O}=0.253$ mol.

Answer:

equal to 0.253 mol.