Question

03 question (1 point)
hcl reacts with nh₃ according to the balanced equation below.
hcl + nh₃ → nh₄cl
0.132 moles of hcl are reacted with 0.411 moles of nh₃.
1st attempt
when 0.132 moles of hcl reacts with 0.411 moles of nh₃, how much nh₃ is consumed?
mol nh₃

Explanation:

Step1: Analyze the reaction ratio

The balanced equation is $HCl + NH_3
ightarrow NH_4Cl$. The mole - ratio of $HCl$ to $NH_3$ is 1:1.

Step2: Determine the limiting reactant

We have 0.132 moles of $HCl$ and 0.411 moles of $NH_3$. Since the mole - ratio of $HCl$ to $NH_3$ is 1:1, $HCl$ is the limiting reactant.

Step3: Calculate the amount of $NH_3$ consumed

Based on the 1:1 mole - ratio, the amount of $NH_3$ consumed is equal to the amount of $HCl$ that reacts. So, the amount of $NH_3$ consumed is 0.132 moles.

Answer:

0.132