(A) Given: $n = 3 \ mol$,$q_p = \Delta H = 229 \ J$,$\Delta T = 2.55 \ K$. At constant pressure,$\Delta H = n \times C_p \times \Delta T$. $C_p = \fra

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(A) Given: $n = 3 \ mol$,$q_p = \Delta H = 229 \ J$,$\Delta T = 2.55 \ K$. At constant pressure,$\Delta H = n \times C_p \times \Delta T$. $C_p = \frac{229}{3 \times 2.55} \approx 29.93 \ J \ K^{-1} \ mol^{-1} \approx 30 \ J \ K^{-1} \ mol^{-1}$. For an ideal gas,$C_v = C_p - R$. Using $R = 8.314 \ J \ K^{-1} \ mol^{-1}$,$C_v = 30 - 8.314 = 21.686 \ J \ K^{-1} \ mol^{-1} \approx 21.7 \ J \ K^{-1} \ mol^{-1}$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

When $3 \ mol$ of $Ar_{(g)}$ is supplied with $229 \ J$ of heat at constant pressure,the temperature of the sample increases by $2.55 \ K$. Calculate the molar heat capacity of the gas at constant volume.

A
$21.7 \ J \ K^{-1} \ mol^{-1}$
B
$30.7 \ J \ K^{-1} \ mol^{-1}$
C
$14.7 \ J \ K^{-1} \ mol^{-1}$
D
$16.7 \ J \ K^{-1} \ mol^{-1}$

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MediumAP EAMCET 2024

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When $3 \ mol$ of $Ar_{(g)}$ is supplied with $229 \ J$ of heat at constant pressure,the temperature of the sample increases by $2.55 \ K$. Calculate the molar heat capacity of the gas at constant volume.

Similar Questions

How much $kJ$ energy is released when $6 \ mol$ of octane is burnt in air? Given $\Delta H_f^o$ for $CO_{2(g)}$,$H_2O_{(g)}$ and $C_8H_{18(l)}$ respectively are $-490$,$-240$,and $+160 \ kJ/mol$.

Consider the reaction at $300 \ K$: $H_{2(g)} + Cl_{2(g)} \to 2HCl_{(g)}$; $\Delta H^o = -185 \ kJ$. If $2 \ mole$ of $H_2$ completely react with $2 \ mole$ of $Cl_2$ to form $HCl$,what is $\Delta U^o$ for this reaction in $kJ$?

Calculate $\Delta S_{total}$ for the following reaction at $300 \ K$. $NH_4NO_{3(s)} \longrightarrow NH_4^+{(aq)} + NO_3^-{(aq)}$ $(\Delta H = 28.1 \ kJ \ mol^{-1}, \Delta S_{sys} = 108.7 \ J \ K^{-1} \ mol^{-1})$

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Calculate $\Delta S_{total}$ for the following reaction at $300 \ K$.
$NH_4NO_{3(s)} \longrightarrow NH_4^+{(aq)} + NO_3^-{(aq)}$ $(\Delta H = 28.1 \ kJ \ mol^{-1}, \Delta S_{sys} = 108.7 \ J \ K^{-1} \ mol^{-1})$

Observe the following reactions:
$AB_{(g)} + 25 H_2O_{(l)} \rightarrow AB_{(25 H_2O)} ; \Delta H = x \ kJ \ mol^{-1}$
$AB_{(g)} + 50 H_2O_{(l)} \rightarrow AB_{(50 H_2O)} ; \Delta H = y \ kJ \ mol^{-1}$
The enthalpy of dilution $(\Delta H_{dil})$ in $kJ \ mol^{-1}$ is