Answer
The chemical equation for the reaction:
$2AgNO_3\rightarrow 2Ag+2NO_2+O_2$
The percent yield=95.27%
Work Step by Step
The molar mass of silver nitrate=169.87amu
The molar mass of Silver=107.8682amu
We calculate the number of moles of silver nitrate using the formula:
Number of moles=$\frac{mass}{molarmass}=\frac{1.099}{169.87}\approx0.00647mol$
we then write a balanced chemical reaction for the decomposition of Silver nitrate to Silver, nitrogen dioxide, and oxygen:
$2AgNO_3\rightarrow 2Ag+2NO_2+O_2$
According to the balanced chemical reaction, 2 moles of silver nitrate produces two moles of silver. So, 0.00647mol silver nitrate will produce 0.00647mol silver.
We can calculate the theoretical mass of silver using the formula:
mass=Number of moles$\times$molar mass of silver=$0.00647\times107.8682\approx0.698g$
Percent yield=$\frac{\text{Actual yield}}{\text{theoritical yield}}\times100=\frac{0.665}{0.698}\times100\approx95.27\%$
