the following balanced equation shows the formation of water.\n2h₂ + o₂ → 2h₂o\nhow many moles of oxygen…

the following balanced equation shows the formation of water.\n2h₂ + o₂ → 2h₂o\nhow many moles of oxygen (o₂) are required to completely react with 27.4 mol of h₂?\no 6.8 mol\no 13.7 mol\no 54.8 mol\no 109.6 mol

the following balanced equation shows the formation of water.\n2h₂ + o₂ → 2h₂o\nhow many moles of oxygen (o₂) are required to completely react with 27.4 mol of h₂?\no 6.8 mol\no 13.7 mol\no 54.8 mol\no 109.6 mol

Answer

Explanation:

Step1: Identify mole - ratio

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

Step2: Set up proportion

Let $x$ be the number of moles of $O_2$. We have the proportion $\frac{2\ mol\ H_2}{1\ mol\ O_2}=\frac{27.4\ mol\ H_2}{x}$.

Step3: Solve for $x$

Cross - multiply: $2x = 27.4\times1$. Then $x=\frac{27.4}{2}=13.7\ mol$.

Answer:

B. 13.7 mol