Question

Please help. What mass of copper is required to replace silver from 4.00g of silver nitrate dissolved in water? I found the molar mass of all of them but don't know where to go from there

Answer 1

0.7479 grams of copper is required to replace 4.00 grams of silver nitrate.

Step-by-step explanation:

`Cu+2AgNO_3\rightarrow Cu(NO_3)_2+2Ag`

Moles of silver nitrate =
`(4.00 g)/(169.87 g/mol)=0.0235 mol`

According to reaction 2 moles of silver nitrate reacts with 1 mole of copper metal.

Then 0.02354 moles of silver nitrate will react with:

`(1)/(2)* 0.0235 mol=0.01177 mol`

Mass of 0.01177 moles copper =0.01177 mol × 63.55 g/mol = 0.7479 g

0.7479 grams of copper is required to replace 4.00 grams of silver nitrate.

Answer 2

It's importaint to first set up the equation. 2AgNO3+Cu--->Cu(NO3)2+2Ag this will dtermine whether you need to divide by two when you divide the moler mass of silver nitrate with 4g to find the amout of moles.023547419, then you divide by two and multiply by the molor mass of CU(NO3)2 and you should get your answer. I got 2.208grams. (please tell me if i'm wrong, going to be an AP Chemistry student.), i copyed myself so don't ban me.