In the synthesis of ammonium nitrate, the reaction is $\mathrm{NH_3(g) + HNO_3(aq) - NH_4NO_3(aq)}$. A student mixes 2.00 g of $\mathrm{NH_3}$ (M = 17.03 g mol^{-1}) with 3.00 g of $\mathrm{HNO_3}$ (M = 63.01 g mol^{-1}). After the reaction, 3.20 g of solid $\mathrm{NH_4NO_3}$ is obtained. (a) Identify the limiting reagent. (b) Calculate the theoretical yield of $\mathrm{NH_4NO_3}$. (c) Determine the percent yield.

Question

In the synthesis of ammonium nitrate, the reaction is $\mathrm{NH_3(g) + HNO_3(aq) -> NH_4NO_3(aq)}$. A student mixes 2.00 g of $\mathrm{NH_3}$ (M = 17.03 g mol^{-1}) with 3.00 g of $\mathrm{HNO_3}$ (M = 63.01 g mol^{-1}). After the reaction, 3.20 g of solid $\mathrm{NH_4NO_3}$ is obtained. (a) Identify the limiting reagent. (b) Calculate the theoretical yield of $\mathrm{NH_4NO_3}$. (c) Determine the percent yield.

Accepted Answer

Limiting reagent: HNO₃; Theoretical yield: 3.81 g; Percent yield: 84.0%

Neco 2025 Chemistry Question 5

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