Answer: approximately 74 milliliters (mL) of 1.42 M copper nitrate would be produced when copper metal reacts with 300 mL of 0.7 M silver nitrate.
Explanation: Cu + AgNO3 → Cu(NO3)2 + Ag
The balanced equation shows that 1 mole of copper reacts with 2 moles of silver nitrate to produce 1 mole of copper nitrate and 1 mole of silver.
Given:
Volume of silver nitrate solution (V1) = 300 mL
Molarity of silver nitrate solution (M1) = 0.7 M
Molarity of copper nitrate solution (M2) = 1.42 M
To find the number of moles of silver nitrate used, we can use the formula:
moles of silver nitrate (n1) = Molarity (M1) × Volume (V1)
= 0.7 mol/L × 0.3 L
= 0.21 moles
According to the balanced equation, 2 moles of silver nitrate react to produce 1 mole of copper nitrate. Therefore, the number of moles of copper nitrate (n2) produced is:
moles of copper nitrate (n2) = 0.21 moles ÷ 2
= 0.105 moles
Now, let's calculate the volume of the copper nitrate solution using the formula:
Volume (V2) = moles (n2) ÷ Molarity (M2)
= 0.105 moles ÷ 1.42 mol/L
≈ 0.074 L
≈ 74 mL