Questions: How many moles of ammonia would be required to react exactly with 0.366 moles of copper(II) oxide in the following chemical reaction? 2 NH3(g) + 3 CuO(s) → 3 Cu(s) + N2(g) + 3 H2O(g)

Solution Steps

From the balanced chemical equation: \[ 2 \mathrm{NH}_{3}(\mathrm{~g}) + 3 \mathrm{CuO}(\mathrm{~s}) \rightarrow 3 \mathrm{Cu}(\mathrm{~s}) + \mathrm{N}_{2}(\mathrm{~g}) + 3 \mathrm{H}_{2} \mathrm{O}(\mathrm{~g}) \] we see that 2 moles of ammonia (\(\mathrm{NH}_3\)) react with 3 moles of copper(II) oxide (\(\mathrm{CuO}\)).

Given that we have 0.366 moles of \(\mathrm{CuO}\), we need to find how many moles of \(\mathrm{NH}_3\) are required. Using the stoichiometric ratio from the balanced equation: \[ \frac{2 \text{ moles } \mathrm{NH}_3}{3 \text{ moles } \mathrm{CuO}} \] we can set up the proportion: \[ \frac{2 \text{ moles } \mathrm{NH}_3}{3 \text{ moles } \mathrm{CuO}} = \frac{x \text{ moles } \mathrm{NH}_3}{0.366 \text{ moles } \mathrm{CuO}} \]

Solving for \(x\): \[ x = \frac{2}{3} \times 0.366 = 0.244 \text{ moles } \mathrm{NH}_3 \]

Final Answer