Final answer:
To react with 0.5 g of copper metal, 0.01884 mL of 16 M HNO₃ is required.
Step-by-step explanation:
To find the volume of 16 M HNO₃ required to react with 0.5 g of copper metal, we need to use the balanced chemical equation:
3Cu + 8HNO₃ → 3Cu(NO₃)₂ + 4H₂O + 2NO
From the equation, we can see that 3 moles of copper react with 8 moles of HNO₃.
First, calculate the moles of copper using its molar mass (63.55 g/mol):
Moles of copper = Mass of copper / Molar mass of copper = 0.5 g / 63.55 g/mol = 0.007876 mol
Since the ratio of moles of copper to moles of HNO₃ is 3:8, we can calculate the moles of HNO₃:
Moles of HNO₃ = Moles of copper x (8 moles HNO₃ / 3 moles copper) = 0.007876 mol x (8 mol HNO₃ / 3 mol copper) = 0.0210 mol HNO₃
To find the volume of HNO₃, we can use the formula:
Volume (L) = Moles / Molarity
Volume of 16 M HNO₃ = 0.0210 mol / 16 M = 0.001884 L = 0.01884 mL