Question

Hydrogen and oxygen react to produce water according to the following equation.2h2 + o2 2h20
The molar mass of hydrogen gas (h2 ) is 2g . The molar mass of oxygen gas (o2 ) is . 32 g
When the reaction starts with grams of oxygen and a sufficient quantity of hydrogen, how many moles of water are produced?
64
8
4
18
2

Answer 1

To determine how many moles of water are produced when starting with a certain amount of oxygen and sufficient hydrogen, we can use the balanced chemical equation:

\[ 2 \text{H}_2 + \text{O}_2 \rightarrow 2 \text{H}_2\text{O} \]

From the balanced equation, we can see the following ratios:
- 1 mole of \( \text{O}_2 \) produces 2 moles of \( \text{H}_2\text{O} \).

Next, we need to calculate the number of moles of \( \text{O}_2 \) available. The molar mass of \( \text{O}_2 \) is given as 32 g. If we assume we start with 64 grams of \( \text{O}_2 \):

\[
\text{Moles of } \text{O}_2 = \frac{\text{mass}}{\text{molar mass}} = \frac{64 \text{ g}}{32 \text{ g/mol}} = 2 \text{ moles of } \text{O}_2
\]

Since 1 mole of \( \text{O}_2 \) produces 2 moles of \( \text{H}_2\text{O} \):

\[
2 \text{ moles of } \text{O}_2 \times 2 = 4 \text{ moles of } \text{H}_2\text{O}
\]

Therefore, starting with 64 grams of oxygen and a sufficient amount of hydrogen, you would produce **4 moles of water**.

Thus, the answer is **4**.