Respuesta :
Answer: The mass of silver nitrate that must be dissolved is 1.58 grams.
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] ......(1)
Given mass of silver = 1 g
Molar mass of silver = 107.86 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of silver}=\frac{1g}{107.86g/mol}=0.0093mol[/tex]
The chemical equation for the reaction of silver nitrate and copper follows:
[tex]2AgNO_3+Cu\rightarrow Cu(NO_3)_2+2Ag[/tex]
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 = [tex]\frac{2}{2}\times 0.0093=0.0093moles[/tex] 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:
[tex]0.0093mol=\frac{\text{Mass of silver nitrate}}{169.87g/mol}\\\\\text{Mass of silver nitrate}=1.58g[/tex]
Hence, the mass of silver nitrate that must be dissolved is 1.58 grams.
