First we need to find how many moles are in the sample of silver of the problem.
The molar mass of silver is [tex]M_m = 107.9 g/mol[/tex]. This means that in m=9.50 g of silver we have
[tex]n= \frac{m}{M_m}= \frac{9.5 g}{107.9 g/mol}=0.088 mol [/tex]
Now we can calculate the energy needed to raise the temperature of this amount of silver by [tex]16.8 ^{\circ}[/tex]:
[tex]Q= n C_m \Delta T=(0.088 mol)(25.35 J/mol ^{\circ} C)(16.8^{\circ}C)=37.5 J [/tex]
