Question

1. the unbalanced chemical equation below represents the formation of ammonia.

n₂(g) + h₂(g) → __ nh₃(g)
when the equation is balanced using the smallest whole - number coefficients, what is the ratio of moles of hydrogen consumed to moles of ammonia produced?
1:3
3:2
3:1
2:3
clear all

Explanation:

Step1: Balance the chemical equation

The unbalanced equation is \( \text{N}_2(g) + \text{H}_2(g)
ightarrow \text{NH}_3(g) \).

• For nitrogen: There are 2 N atoms on the left, so we need 2 \( \text{NH}_3 \) on the right. Now the equation becomes \( \text{N}_2 + \text{H}_2

ightarrow 2\text{NH}_3 \).

• For hydrogen: There are \( 2 \times 3 = 6 \) H atoms on the right, so we need \( \frac{6}{2} = 3 \) \( \text{H}_2 \) on the left.

The balanced equation is \( \text{N}_2(g) + 3\text{H}_2(g)
ightarrow 2\text{NH}_3(g) \).

Step2: Determine the ratio

From the balanced equation, moles of \( \text{H}_2 \) consumed = 3, moles of \( \text{NH}_3 \) produced = 2. Wait, no—wait, the question asks for hydrogen consumed to ammonia produced. Wait, no, let's check again. Wait, the balanced equation is \( \text{N}_2 + 3\text{H}_2
ightarrow 2\text{NH}_3 \). So moles of \( \text{H}_2 \) is 3, moles of \( \text{NH}_3 \) is 2? Wait, no, the options include 3:2? Wait, no, the original options: the selected one was 3:1, but let's recalculate. Wait, no, maybe I made a mistake. Wait, the reaction is \( \text{N}_2 + 3\text{H}_2
ightarrow 2\text{NH}_3 \). So moles of \( \text{H}_2 \) is 3, moles of \( \text{NH}_3 \) is 2. But the options have 3:2? Wait, no, the question is ratio of moles of hydrogen consumed to moles of ammonia produced. So \( \frac{\text{moles of } \text{H}_2}{\text{moles of } \text{NH}_3} = \frac{3}{2} \)? Wait, no, wait the balanced equation: \( \text{N}_2 + 3\text{H}_2
ightarrow 2\text{NH}_3 \). So hydrogen is 3, ammonia is 2. So ratio is 3:2. Wait, but the selected option was 3:1. Wait, maybe I messed up. Wait, no—wait, the problem says "ratio of moles of hydrogen consumed to moles of ammonia produced". So hydrogen is 3, ammonia is 2. So 3:2. Wait, but let's rebalance.

Wait, \( \text{N}_2 \) has 2 N, so \( 2\text{NH}_3 \) gives 2 N. Then \( 2\text{NH}_3 \) has 6 H, so \( 3\text{H}_2 \) (since each \( \text{H}_2 \) has 2 H, 3*2=6). So balanced equation: \( \text{N}_2 + 3\text{H}_2
ightarrow 2\text{NH}_3 \). So moles of \( \text{H}_2 \) is 3, moles of \( \text{NH}_3 \) is 2. So ratio of \( \text{H}_2 \) to \( \text{NH}_3 \) is 3:2. Wait, but the options include 3:2. So the correct ratio is 3:2. Wait, maybe the initial selected option was wrong. Let's check the options again. The options are 1:3, 3:2, 3:1, 2:3. So according to the balanced equation, \( \text{H}_2 \) is 3, \( \text{NH}_3 \) is 2, so ratio 3:2.

Wait, I think I made a mistake earlier. So the correct ratio is 3:2.

Answer:

3:2 (So the correct option is the one with 3:2, i.e., the option labeled "3:2")