Pressurized metal gas cylinders are generally used to store commonly used gases in the laboratory. At times, it can be easier to chemically prepare occasionally used gases. For example, nitrogen monoxide, NO(g) , can be prepared in the lab by the following chemical reaction:
3Cu(s) + 8HNO₃(aq) $\rarr$ 2NO(g) + 3Cu(NO₃) ₂(aq) + 4H₂O(l)
If 15 g of copper metal was added to an aqueous solution containing 6.0 moles of HNO₃, how many moles of NO(g) would be produced, assuming a 75% yield

Question

Pressurized metal gas cylinders are generally used to store commonly used gases in the laboratory. At times, it can be easier to chemically prepare occasionally used gases. For example, nitrogen monoxide, NO(g) , can be prepared in the lab by the following chemical reaction:
3Cu(s) + 8HNO₃(aq)

\rarr

2NO(g) + 3Cu(NO₃) ₂(aq) + 4H₂O(l)
If 15 g of copper metal was added to an aqueous solution containing 6.0 moles of HNO₃, how many moles of NO(g) would be produced, assuming a 75% yield

Quizplus · Accepted Answer

First, calculate the moles of copper (Cu) used. The molar mass of Cu is approximately 63.55 g/mol. For 15 g of Cu: $ \frac{15 \, \text{g}}{63.55 \, \text{g/mol}} = 0.236 \, \text{mol} \, \text{Cu} $. According to the balanced chemical equation, 3 moles of Cu produce 2 moles of NO. Therefore, $ 0.236 \, \text{mol} \, \text{Cu} $ would produce $ \frac{2}{3} \times 0.236 = 0.157 \, \text{mol} \, \text{NO} $ in a 100% yield. Given a 75% yield, the actual amount of NO produced would be $ 0.157 \, \text{mol} \times 0.75 = 0.118 \, \text{mol} \, \text{NO} $, which rounds to 0.12 mole NO.

Pressurized Metal Gas Cylinders Are Generally Used to Store Commonly →\rarr→

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