How many grams of copper will be required to replace silver from 200 mL of 3.00M solution of silver nitrate AgNO3?
Follow the steps in this example problem.
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To determine how many grams of copper will be required to replace silver from the solution, we need to use the concept of stoichiometry.
First, let's determine the number of moles of silver nitrate in the solution. We can use the formula:
moles = concentration (M) × volume (L)
Given that the concentration of the silver nitrate solution is 3.00 M and the volume is 200 mL (0.200 L), we can calculate the number of moles of silver nitrate:
moles of AgNO3 = 3.00 M × 0.200 L = 0.600 moles
According to the balanced chemical equation for the reaction between copper and silver nitrate (Cu + 2AgNO3 -> Cu(NO3)2 + 2Ag), we can see that 1 mole of copper reacts with 2 moles of silver nitrate.
Therefore, 0.600 moles of silver nitrate would require half as many moles of copper:
moles of Cu = 0.600 moles ÷ 2 = 0.300 moles
To calculate the mass of copper in grams, we need to use the molar mass of copper, which is 63.55 g/mol:
mass of Cu = moles of Cu × molar mass of Cu
mass of Cu = 0.300 moles × 63.55 g/mol = 19.07 grams
Hence, approximately 19.07 grams of copper will be required to replace silver from 200 mL of 3.00 M solution of silver nitrate.