<u>Answer:</u> The mass of silver nitrate that must be dissolved is 1.58 grams.
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
......(1)
Given mass of silver = 1 g
Molar mass of silver = 107.86 g/mol
Putting values in equation 1, we get:
![\text{Moles of silver}=\frac{1g}{107.86g/mol}=0.0093mol](https://tex.z-dn.net/?f=%5Ctext%7BMoles%20of%20silver%7D%3D%5Cfrac%7B1g%7D%7B107.86g%2Fmol%7D%3D0.0093mol)
The chemical equation for the reaction of silver nitrate and copper follows:
![2AgNO_3+Cu\rightarrow Cu(NO_3)_2+2Ag](https://tex.z-dn.net/?f=2AgNO_3%2BCu%5Crightarrow%20Cu%28NO_3%29_2%2B2Ag)
By Stoichiometry of the reaction:
2 moles of silver is produced from 2 moles of silver nitrate
So, 0.0093 moles of silver will be produced from =
of silver nitrate
Now, calculating the mass of silver nitrate from equation 1, we get:
Molar mass of silver nitrate = 169.87 g/mol
Moles of silver nitrate = 0.0093 moles
Putting values in equation 1, we get:
![0.0093mol=\frac{\text{Mass of silver nitrate}}{169.87g/mol}\\\\\text{Mass of silver nitrate}=1.58g](https://tex.z-dn.net/?f=0.0093mol%3D%5Cfrac%7B%5Ctext%7BMass%20of%20silver%20nitrate%7D%7D%7B169.87g%2Fmol%7D%5C%5C%5C%5C%5Ctext%7BMass%20of%20silver%20nitrate%7D%3D1.58g)
Hence, the mass of silver nitrate that must be dissolved is 1.58 grams.