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 using the following chemical reaction: 3Cu(s) + 8HNO₃(aq) $\rarr$ 2NO(g) + 3Cu(NO₃) ₂(aq) + 4H₂O(l)
If 5.0 g of copper metal was added to an aqueous solution containing 2.5 moles of HNO₃, how many moles of NO(g) would be produced, assuming a 100% 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 using the following chemical reaction: 3Cu(s) + 8HNO₃(aq)

\rarr

2NO(g) + 3Cu(NO₃) ₂(aq) + 4H₂O(l)
If 5.0 g of copper metal was added to an aqueous solution containing 2.5 moles of HNO₃, how many moles of NO(g) would be produced, assuming a 100% yield

Quizplus · Accepted Answer

First, we need to balance the chemical equation. 3Cu(s) + 8HNO₃(aq) → 2NO(g) + 3Cu(NO₃)₂(aq) + 4H₂O(l) Next, we can use stoichiometry to find the number of moles of NO produced. From the balanced equation, we can see that 3 moles of Cu reacts with 8 moles of HNO₃(aq) to produce 2 moles of NO. Moles of HNO₃(aq) = concentration x volume = 2.5 mol/L x 1 L = 2.5 mol Moles of Cu = 5.0 g / 63.55 g/mol = 0.079 mol Using the mole ratio from the balanced equation: 0.079 mol Cu x (2 mol NO / 3 mol Cu) = 0.053 mol NO Since the reaction is assumed to have a 100% yield, the answer is 0.053 mol NO, which is closest to option B (0.052 mole NO).

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

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