Question

Hydrogen and oxygen react to produce water according to the following equation.

2H2+O2→2H2O

The molar mass of hydrogen gas (H2
) is 2 g/mol
. The molar mass of oxygen gas (O2
) is 32 g/mol
. When the reaction starts with 64
grams of oxygen and a sufficient quantity of hydrogen, how many moles of water are produced?

(1 point)
Responses

8
8

18
18

2
2

4
4

Answer 1

To determine how many moles of water are produced in the reaction given the starting amount of oxygen, we can follow these steps:

1. **Calculate the moles of oxygen**:
\[
\text{Moles of } O_2 = \frac{\text{mass of } O_2}{\text{molar mass of } O_2} = \frac{64 \text{ g}}{32 \text{ g/mol}} = 2 \text{ moles of } O_2
\]

2. **Use the stoichiometry of the reaction**: According to the balanced equation:
\[
2H_2 + O_2 \rightarrow 2H_2O
\]
This shows that 1 mole of \( O_2 \) produces 2 moles of \( H_2O \).

3. **Calculate moles of water produced**:
Since we have 2 moles of \( O_2 \), the amount of water produced would be:
\[
\text{Moles of } H_2O = 2 \text{ moles of } O_2 \times 2 = 4 \text{ moles of } H_2O
\]

Therefore, the answer is **4 moles of water** produced.