Questions: QUESTION 8 Ammonium nitrate fertilizer is sometimes used as an explosive. How many moles of water can be formed from the decomposition of 13.2 moles of ammonium nitrate? a. 26.4 mol 2 NH4NO3 → 2 N2+O2+4 H2O b. 14.0 mol c. 13.2 mol d. 18.0 mol e. 6.60 mol

QUESTION 8 Ammonium nitrate fertilizer is sometimes used as an explosive. How many moles of water can be formed from the decomposition of 13.2 moles of ammonium nitrate? a. 26.4 mol 2 NH4NO3 → 2 N2+O2+4 H2O b. 14.0 mol c. 13.2 mol d. 18.0 mol e. 6.60 mol

Transcript text: QUESTION 8 Ammonium nitrate fertilizer is sometimes used as an explosive. How many moles of water can be formed from the decomposition of 13.2 moles of ammonium nitrate? a. 26.4 mol \[ 2 \mathrm{NH}_{4} \mathrm{NO}_{3} \rightarrow 2 \mathrm{~N}_{2}+\mathrm{O}_{2}+4 \mathrm{H}_{2} \mathrm{O} \] b. 14.0 mol c. 13.2 mol d. 18.0 mol e. 6.60 mol

Solution

Solution Steps

Step 1: Understand the Chemical Reaction

The decomposition reaction of ammonium nitrate is given by:

\[ 2 \mathrm{NH}_{4} \mathrm{NO}_{3} \rightarrow 2 \mathrm{~N}_{2}+\mathrm{O}_{2}+4 \mathrm{H}_{2} \mathrm{O} \]

This equation shows that 2 moles of ammonium nitrate produce 4 moles of water.

Step 2: Determine the Mole Ratio

From the balanced chemical equation, the mole ratio of ammonium nitrate to water is:

\[ \frac{4 \text{ moles of } \mathrm{H}_{2}\mathrm{O}}{2 \text{ moles of } \mathrm{NH}_{4}\mathrm{NO}_{3}} = 2 \]

This means that for every 1 mole of ammonium nitrate, 2 moles of water are produced.

Step 3: Calculate the Moles of Water Formed

Given that we have 13.2 moles of ammonium nitrate, we can calculate the moles of water produced using the mole ratio:

\[ \text{Moles of } \mathrm{H}_{2}\mathrm{O} = 13.2 \text{ moles of } \mathrm{NH}_{4}\mathrm{NO}_{3} \times 2 = 26.4 \text{ moles of } \mathrm{H}_{2}\mathrm{O} \]