(B) For an adiabatic process,the work done is given by the change in internal energy: $W = \Delta U = nC_v(T_2 - T_1)$.Given: $n = 1\, mol$,$C_v = 20\

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(B) For an adiabatic process,the work done is given by the change in internal energy: $W = \Delta U = nC_v(T_2 - T_1)$.Given: $n = 1\, mol$,$C_v = 20\, J/K$,$T_1 = 27 + 273 = 300\, K$,and $W = -3000\, J$ (work done by the system is negative).Substituting the values: $-3000 = 1 \times 20 \times (T_2 - 300)$.$-150 = T_2 - 300$.$T_2 = 300 - 150 = 150\, K$.

Class 11 Chemistry Thermodynamics First law of thermodynamics

Medium

One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of $27\,^{\circ}C$. If the work done during the process is $3\, kJ$,then the final temperature of the gas is $(C_v = 20\, J/K)$ .....$K$

A
$100$
B
$150$
C
$195$
D
$255$

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Thermodynamics

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First law of thermodynamics

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One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of $27\,^{\circ}C$. If the work done during the process is $3\, kJ$,then the final temperature of the gas is $(C_v = 20\, J/K)$ .....$K$

Similar Questions

$A$ gas absorbs $150 \ J$ of heat and expands by $300 \ cm^3$ against a constant external pressure of $2 \times 10^5 \ N \ m^{-2}$. What is the change in internal energy $(\Delta U)$ of the system (in $J$)?

According to the first law of thermodynamics,which of the following is correct? (Where $q =$ heat supplied to the system and $W =$ work done by the system)

In the complete combustion of butanol $C_4H_9OH_{(l)}$,if $\Delta H$ is the enthalpy of combustion and $\Delta E$ is the heat of combustion at constant volume,then

Calculate the internal energy change of a system if the work done by the system is $8 \ J$ and the heat supplied to it is $40 \ J$. (in $J$)

$A$ system is provided $50 \text{ J}$ of heat and work done on the system is $10 \text{ J}$. What is the change in internal energy (in $\text{ J}$)?

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