Question

For silver, $C_p\left(J{K}^{-1}mo{l}^{-1}\right)=23+0.01T$. If the temperature $\text{(T)}$ of moles of silver is raised from $300\text{K}$ to $1000\text{K}$ at $1\text{atm}$ pressure, the value of $\Delta H$ will be close to:

• A. $13\text{kJ}$
• B. $16\text{kJ}$
• C. $21\text{kJ}$
• D. $62\text{kJ}$

Answer 1

The correct option is D $62\text{kJ}$

$\text{Given}:\text{n = 3}$
$T_1=300;T_2=1000$

$C_p=23+0.01T$

$\Delta Hand{C}_p$

$\Delta H=\underset{T_1}{\overset{T_2}{\int }}n{C}_{p}dT$

$\Delta H=n\underset{300}{\overset{1000}{\int }}\left(\mathrm{23.0.01}T\right)dT$

$=3\left[23\right(1000-300\left)\right[+\frac{0.01}{2}({1000}^2-{300}^2)\left]\right]$

$=3[16100+4550]$

$=61.95kJ$

$=3\times 20650=61950J$

$\approx 62\text{kJ}$