How many grams of copper will be required to replace silver from 200 mL of 3.00M solution of silver nitrate AgNO3?
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To determine the number of grams of copper required to replace silver from the solution, we need to use the concept of stoichiometry and calculate the molar ratio between copper and silver in the reaction. Here are the steps to find the answer:
Step 1: Write the balanced chemical equation for the reaction between copper and silver nitrate:
Cu + 2AgNO3 → Cu(NO3)2 + 2Ag
Step 2: Identify the molar ratio between copper (Cu) and silver (Ag) in the balanced equation. In this case, for every 1 mole of copper, 2 moles of silver are required.
Step 3: Calculate the number of moles of silver in the solution:
To find the number of moles, we use the formula:
moles = concentration (in M) × volume (in L)
Given:
Concentration of silver nitrate solution (AgNO3) = 3.00 M
Volume of silver nitrate solution (V) = 200 mL = 200/1000 = 0.2 L
moles of AgNO3 = concentration × volume
= 3.00 M × 0.2 L
= 0.6 moles
Step 4: Calculate the number of moles of copper required using the molar ratio:
From the balanced equation, we know that 2 moles of silver are required for every 1 mole of copper.
moles of Cu = (moles of AgNO3) / 2
= 0.6 moles / 2
= 0.3 moles
Step 5: Calculate the mass of copper required using its molar mass:
The molar mass of copper (Cu) is 63.55 g/mol.
mass of Cu = moles of Cu × molar mass of Cu
= 0.3 moles × 63.55 g/mol
= 19.065 g
Therefore, approximately 19.065 grams of copper would be required to replace the silver from 200 mL of a 3.00M solution of silver nitrate (AgNO3).