(B) For the process $AB$:$\Delta U_{AB} = q_{AB} + W_{AB} = 2 + (-5) = -3 \ kJ \ mol^{-1}$For the cyclic process,the total change in internal energy i

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(B) For the process $AB$:$\Delta U_{AB} = q_{AB} + W_{AB} = 2 + (-5) = -3 \ kJ \ mol^{-1}$For the cyclic process,the total change in internal energy is zero:$\Delta U_{AB} + \Delta U_{BC} + \Delta U_{CA} = 0$Substituting the known values:$-3 + (-5) + \Delta U_{CA} = 0$$\Delta U_{CA} = 8 \ kJ \ mol^{-1}$Using the first law of thermodynamics for process $CA$:$\Delta U_{CA} = q_{CA} + W_{CA}$$8 = q_{CA} + 3$$q_{CA} = 5 \ kJ \ mol^{-1}$Thus,the heat absorbed by the system during process $CA$ is $+5 \ kJ \ mol^{-1}$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

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An ideal gas undergoes a cyclic process as shown in the figure.
$\Delta U_{BC} = -5 \ kJ \ mol^{-1}$,$q_{AB} = 2 \ kJ \ mol^{-1}$
$\Delta W_{AB} = -5 \ kJ \ mol^{-1}$,$W_{CA} = 3 \ kJ \ mol^{-1}$
Heat absorbed by the system during process $CA$ is......$kJ \ mol^{-1}$

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A
$-5$
B
$+5$
C
$18$
D
$-18$

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Consider the following statements:
Statement-$I$: During isothermal expansion of an ideal gas,its enthalpy decreases.
Statement-$II$: When $2.0 \ L$ of an ideal gas expands isothermally into vacuum,$\Delta U = 0$.

MediumAP EAMCET 2025

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When $50 \ cm^3$ of $0.2 \ N \ H_2SO_4$ is mixed with $50 \ cm^3$ of $1 \ N \ KOH$,the heat liberated is

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$18 \ g$ glucose is completely combusted in a bomb calorimeter of heat capacity $1400 \ kJ/K$. The temperature changes from $27 \ ^\circ C$ to $27.2 \ ^\circ C$. Calculate the magnitude of the standard enthalpy of combustion of glucose in $kJ/mol$. $[R = 8.314 \ J/mol-K]$

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Calculate the work done during the combustion of $0.138 \ kg$ of ethanol,$(C_2H_5OH_{(l)})$ at $300 \ K$. Given: $R = 8.314 \ J \ K^{-1} \ mol^{-1}$ and molar mass of ethanol $= 46 \ g \ mol^{-1}$. (in $J$)

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The enthalpy of dilution of $4 \ M \ HCl$ to $2 \ M \ HCl$ is $-2.5 \ kJ/mol$. Find the enthalpy change when $500 \ mL$ of $4 \ M \ HCl$ is diluted to $2 \ M \ HCl$ (in $kJ$).

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An ideal gas undergoes a cyclic process as shown in the figure.$\Delta U_{BC} = -5 \ kJ \ mol^{-1}$,$q_{AB} = 2 \ kJ \ mol^{-1}$$\Delta W_{AB} = -5 \ kJ \ mol^{-1}$,$W_{CA} = 3 \ kJ \ mol^{-1}$Heat absorbed by the system during process $CA$ is......$kJ \ mol^{-1}$

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Consider the following statements:Statement-$I$: During isothermal expansion of an ideal gas,its enthalpy decreases.Statement-$II$: When $2.0 \ L$ of an ideal gas expands isothermally into vacuum,$\Delta U = 0$.

When $50 \ cm^3$ of $0.2 \ N \ H_2SO_4$ is mixed with $50 \ cm^3$ of $1 \ N \ KOH$,the heat liberated is

$18 \ g$ glucose is completely combusted in a bomb calorimeter of heat capacity $1400 \ kJ/K$. The temperature changes from $27 \ ^\circ C$ to $27.2 \ ^\circ C$. Calculate the magnitude of the standard enthalpy of combustion of glucose in $kJ/mol$. $[R = 8.314 \ J/mol-K]$

Calculate the work done during the combustion of $0.138 \ kg$ of ethanol,$(C_2H_5OH_{(l)})$ at $300 \ K$. Given: $R = 8.314 \ J \ K^{-1} \ mol^{-1}$ and molar mass of ethanol $= 46 \ g \ mol^{-1}$. (in $J$)

The enthalpy of dilution of $4 \ M \ HCl$ to $2 \ M \ HCl$ is $-2.5 \ kJ/mol$. Find the enthalpy change when $500 \ mL$ of $4 \ M \ HCl$ is diluted to $2 \ M \ HCl$ (in $kJ$).

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An ideal gas undergoes a cyclic process as shown in the figure.
$\Delta U_{BC} = -5 \ kJ \ mol^{-1}$,$q_{AB} = 2 \ kJ \ mol^{-1}$
$\Delta W_{AB} = -5 \ kJ \ mol^{-1}$,$W_{CA} = 3 \ kJ \ mol^{-1}$
Heat absorbed by the system during process $CA$ is......$kJ \ mol^{-1}$

Consider the following statements:
Statement-$I$: During isothermal expansion of an ideal gas,its enthalpy decreases.
Statement-$II$: When $2.0 \ L$ of an ideal gas expands isothermally into vacuum,$\Delta U = 0$.