when copper metal is added to silver nitrate in solution, silver metal and copper (II) nitrate are produced. if 1.00*10^2g of copper metal is added to the solution containing 1000.0 g of silver nitrate, what mass of silver metal will be produced?
write the balanced equation for the reaction.
Convert those masses to moles
see which reagent is exhausted first. That will determine how many moles of product are produced.
Then convert back to grams.
To find the mass of silver metal produced, we need to use stoichiometry and balance the chemical equation for the reaction between copper metal (Cu) and silver nitrate (AgNO3).
The balanced chemical equation is:
Cu + 2AgNO3 -> 2Ag + Cu(NO3)2
From the balanced equation, we can see that 1 mole of Cu reacts with 2 moles of AgNO3 to produce 2 moles of Ag.
To solve the problem, follow these steps:
Step 1: Convert the mass of copper (Cu) to moles.
- The molar mass of copper (Cu) is 63.55 g/mol.
- Use the formula: moles = mass / molar mass
- Calculate: moles of Cu = 1.00*10^2 g / 63.55 g/mol
Step 2: Use the mole ratio from the balanced equation to determine the moles of silver (Ag) produced.
- From the balanced equation: 1 mole Cu reacts with 2 moles Ag.
- Use the mole ratio: moles of Ag = moles of Cu * (2 moles Ag / 1 mole Cu)
Step 3: Convert the moles of silver (Ag) to mass.
- The molar mass of silver (Ag) is 107.87 g/mol.
- Use the formula: mass = moles * molar mass
- Calculate: mass of Ag = moles of Ag * 107.87 g/mol
Now, let's perform the calculations:
Step 1:
moles of Cu = 1.00*10^2 g / 63.55 g/mol
Step 2:
moles of Ag = moles of Cu * (2 moles Ag / 1 mole Cu)
Step 3:
mass of Ag = moles of Ag * 107.87 g/mol
By performing these calculations, you will find the mass of silver (Ag) produced.