JEE Mains · Chemistry · STD 11 - 5. Thermodynamics and thermochemistry
For silve \({C_P}\,\left( {J{K^{ - 1}}\,mo{l^{ - 1}}} \right) = 23 + 0.01\,T\) . 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.....\(kJ\)
- A \(13\)
- B \(62\)
- C \(16\)
- D \(21\)
Answer & Solution
Correct Answer
(B) \(62\)
Step-by-step Solution
Detailed explanation
\(\Delta H = n\int\limits_{{T_1}}^{{T_2}} {{C_{p.m}}dT = 3 \times \int\limits_{300}^{1000} {(23 + 0.01\,T)} } dT\) \( = 3[23(1000 - 300)] + \frac{{0.01}}{2}[{(1000)^2} - {(300)^2}]\) \( = 61950\,J \approx 62\,kJ\)
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