For silver,C_P , (J , K^{-1} , mol^{-1}) = 23 | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) The change in enthalpy $(\Delta H)$ for a process at constant pressure is given by the integral of $n \, C_P \, dT$. Given $n = 3 \, mol$,$C_P = 2

Vedclass · Accepted Answer

$62$

Vedclass · Answer

(B) The change in enthalpy $(\Delta H)$ for a process at constant pressure is given by the integral of $n \, C_P \, dT$. Given $n = 3 \, mol$,$C_P = 23 + 0.01 \, T$,$T_1 = 300 \, K$,and $T_2 = 1000 \, K$. $\Delta H = n \int_{T_1}^{T_2} C_P \, dT = 3 \int_{300}^{1000} (23 + 0.01 \, T) \, dT$. $\Delta H = 3 [23 \, T + \frac{0.01 \, T^2}{2}]_{300}^{1000}$. $\Delta H = 3 [23(1000 - 300) + 0.005(1000^2 - 300^2)]$. $\Delta H = 3 [23(700) + 0.005(1000000 - 90000)]$. $\Delta H = 3 [16100 + 0.005(910000)]$. $\Delta H = 3 [16100 + 4550] = 3 [20650] = 61950 \, J$. Converting to $kJ$,$\Delta H = 61.95 \, kJ \approx 62 \, kJ$.

For silver,$C_P \, (J \, K^{-1} \, mol^{-1}) = 23 + 0.01 \, T$. If the temperature $(T)$ of $3 \, moles$ of silver is raised from $300 \, K$ to $1000 \, K$ at $1 \, atm$ pressure,the value of $\Delta H$ will be close to $kJ$.

Similar Questions

Calculate the work done in $kJ$ when $3$ moles of an ideal gas at $27^{\circ} C$ expand isothermally and reversibly from $10 \ atm$ to $1 \ atm$ $[R=8.314 \ J \ K^{-1} \ mol^{-1}]$

Five moles of a gas are subjected to a series of changes as shown in the given graph. What are the processes $A \rightarrow B$,$B \rightarrow C$,and $C \rightarrow A$ respectively?

For the following reaction occurring in automobiles,the values of $\Delta H, \Delta S, \text{and } \Delta G$ are respectively:
$2C_8H_{18(g)} + 25O_2(g) \rightarrow 16CO_2(g) + 18H_2O(g)$

At $25$ $^\circ C$ and $1$ $atm$ pressure,the enthalpies of formation of $C_2H_4(g)$,$CO_2(g)$,and $H_2O(l)$ are $52$,$-394$,and $-286 \, kJ \, mol^{-1}$ respectively. The enthalpy of combustion of $C_2H_4$ is ....... $kJ \, mol^{-1}$.

$\Delta H^o_f$ of water is $-285.5 \, kJ \, mol^{-1}$. If enthalpy of neutralisation of monoacidic strong base is $-57.3 \, kJ \, mol^{-1}$,$\Delta H^o_f$ of $OH^{-}$ ion will be.....$kJ \, mol^{-1}$

Vedclass Test Series

Exam Paper Generator

Online Exam Module