What volume of 17 M nitric acid is required to dissolve 15 g of copper by a reaction for which the products are aqueous copper(II)nitrate,nitric oxide gas,and water? Assume 100% reaction.

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction is: 3Cu + 8HNO3 → 3Cu(NO3)2 + 2NO + 4H2O. The molar mass of copper (Cu) is 63.55 g/mol, so 15 g of Cu is 0.236 mol. According to the equation, 8 moles of HNO3 are needed for 3 moles of Cu, so 0.236 mol of Cu requires 0.629 mol of HNO3. The volume of 17 M HNO3 needed is 0.629 mol / 17 mol/L = 0.037 L or 37 mL.

What Volume of 17 M Nitric Acid Is Required to Dissolve