Calculate the mass of copper needed to displace 5.0g of silver from silver nitrate solution.
Cu+2AgNO3->Cu(NO3)2+2Ag
(Relative atomic masses:Ag=108,Cu=63.5)
I got it to be 3.175g needed.
I can't get 3.175 g. Please post your work. Also, please clarify if the 5.0 is 5.0 g Ag or 5.0 g AgNO3.
To calculate the mass of copper needed to displace 5.0g of silver from silver nitrate solution, we can use the law of conservation of mass. According to the balanced chemical equation provided:
Cu + 2AgNO3 -> Cu(NO3)2 + 2Ag
We can see that 1 mole of copper (Cu) reacts with 2 moles of silver nitrate (AgNO3) to produce 1 mole of copper(II) nitrate (Cu(NO3)2) and 2 moles of silver (Ag).
1. Calculate the number of moles of silver (Ag) in 5.0g of silver (Ag):
Using the atomic mass of silver (Ag) as 108g/mol, we can use the formula:
Number of moles = mass (in grams) / molar mass
Number of moles of Ag = 5.0g / 108g/mol = 0.0463 mol
2. Since the balanced equation shows a 1:2 ratio of Cu to Ag, we need twice the number of moles of Cu.
Number of moles of Cu = 0.0463 mol x 2 = 0.0926 mol
3. Calculate the mass of copper (Cu) needed using the molar mass of copper as 63.5g/mol:
Mass of Cu = number of moles x molar mass
Mass of Cu = 0.0926 mol x 63.5g/mol = 5.8781g ≈ 5.88g
Therefore, the mass of copper needed to displace 5.0g of silver from silver nitrate solution is approximately 5.88g.