calculate the volume in ml of 0.250 M silver nitrate solution required to react completely with a 5.00 g piece of copper
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To calculate the volume of the silver nitrate solution required to react completely with the copper, you need to use the balanced chemical equation for the reaction between silver nitrate (AgNO3) and copper (Cu).
The balanced chemical equation is:
2AgNO3 + Cu → 2Ag + Cu(NO3)2
From the equation, you can see that two moles of silver nitrate react with one mole of copper. To find the volume of the silver nitrate solution, you need to follow these steps:
Step 1: Calculate the number of moles of copper (Cu):
You have 5.00 g of copper. To convert this mass into moles, use the molar mass of copper.
The molar mass of copper (Cu) is approximately 63.55 g/mol.
Moles of Cu = Mass of Cu / Molar mass of Cu
Moles of Cu = 5.00 g / 63.55 g/mol
Step 2: Calculate the number of moles of silver nitrate (AgNO3) needed:
From the balanced chemical equation, you know that 2 moles of AgNO3 react with 1 mole of Cu.
So, Moles of AgNO3 = (moles of Cu) / 2
Step 3: Calculate the volume of the silver nitrate solution (in milliliters, mL):
The molarity (M) of the silver nitrate solution is given as 0.250 M.
Moles of AgNO3 = Molarity (M) × Volume (in liters, L)
Volume (in liters, L) = Moles of AgNO3 / Molarity (M)
However, we need the volume in milliliters (mL), so we need to convert:
Volume (in mL) = Volume (in L) × 1000
Plug the values into the formula to calculate the volume:
Volume (in L) = (Moles of AgNO3) / (Molarity (M))
Volume (in mL) = Volume (in L) × 1000
This will give you the volume of the 0.250 M silver nitrate solution required to react completely with the 5.00 g piece of copper.