QuestionMay 29, 2025

9. Given the balanced equation representing a reaction: 4NH_(3)+5O_(2)arrow 4NO+6H_(2)O How many moles of O_(2) are needed to produce 12.5 moles of H_(2)O Show all work and include units in your final answer. (3 points)

9. Given the balanced equation representing a reaction: 4NH_(3)+5O_(2)arrow 4NO+6H_(2)O How many moles of O_(2) are needed to produce 12.5 moles of H_(2)O Show all work and include units in your final answer. (3 points)
9. Given the balanced equation representing a reaction: 4NH_(3)+5O_(2)arrow 4NO+6H_(2)O How many moles of O_(2) are needed to produce 12.5 moles of H_(2)O Show all work and include units in your final answer. (3 points)

Solution
4.2(425 votes)

Answer

10.42 moles of O_2 (rounded to two decimal places) Explanation 1. Determine Mole Ratio From the balanced equation, the mole ratio of O_2 to H_2O is 5:6. 2. Calculate Moles of O_2 Use the mole ratio to find moles of O_2: \[ \text{Moles of } O_2 = \frac{5}{6} \times 12.5 \] 3. Perform Calculation Calculate: \[ \text{Moles of } O_2 = \frac{5}{6} \times 12.5 = 10.4167 \]

Explanation

1. Determine Mole Ratio<br /> From the balanced equation, the mole ratio of $O_2$ to $H_2O$ is 5:6.<br /><br />2. Calculate Moles of $O_2$<br /> Use the mole ratio to find moles of $O_2$: <br />\[ \text{Moles of } O_2 = \frac{5}{6} \times 12.5 \]<br /><br />3. Perform Calculation<br /> Calculate:<br />\[ \text{Moles of } O_2 = \frac{5}{6} \times 12.5 = 10.4167 \]
Click to rate:

Similar Questions