To find out how many moles of water are produced in the reaction between hydrogen and oxygen, we first need to determine how many moles of oxygen we have based on the provided grams of oxygen.
-
Calculate moles of oxygen: The molar mass of \( O_2 \) (oxygen gas) is given as 32 g/mol. If we have 64 grams of \( O_2 \), we can calculate the moles of oxygen using the formula: \[ \text{moles of } O_2 = \frac{\text{mass (grams)}}{\text{molar mass (g/mol)}} \] Substituting the given values: \[ \text{moles of } O_2 = \frac{64 \text{ g}}{32 \text{ g/mol}} = 2 \text{ moles} \]
-
Use the balanced equation: The balanced chemical equation is: \[ 2H_2 + O_2 \rightarrow 2H_2O \] According to the equation, 1 mole of \( O_2 \) produces 2 moles of \( H_2O \). Since we have 2 moles of \( O_2 \), we can calculate the moles of water produced: \[ \text{moles of } H_2O = 2 \times (\text{moles of } O_2) \] So, \[ \text{moles of } H_2O = 2 \times 2 = 4 \text{ moles} \]
Therefore, starting with 64 grams of oxygen and a sufficient quantity of hydrogen, 4 moles of water are produced.
1 answer