(A) For an adiabatic process,the first law of thermodynamics states that $\Delta U = q + w$. Since $q = 0$,$\Delta U = w$.Given $w = -3\, kJ = -3000\,

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(A) For an adiabatic process,the first law of thermodynamics states that $\Delta U = q + w$. Since $q = 0$,$\Delta U = w$.Given $w = -3\, kJ = -3000\, J$ (work done by the system is negative).We know $\Delta U = n \times C_v \times \Delta T$.Substituting the values: $-3000 = 1 \times 20 \times (T_f - 300)$.$-150 = T_f - 300$.$T_f = 300 - 150 = 150\, K$.

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 $(C_v = 20\, J\, K^{-1}\, mol^{-1})$ .....$K$

A
$150$
B
$450$
C
$1750$
D
$225$

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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 $(C_v = 20\, J\, K^{-1}\, mol^{-1})$ .....$K$

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The reaction in which $\Delta H > \Delta U$ is

Calculate the difference between $\Delta H$ and $\Delta U$ for the combustion of $n$-octane at $25^{\circ}C$. (in $kJ$)

For the reaction $CH_3COOH_{(l)} + 2O_{2(g)} \rightleftharpoons 2CO_{2(g)} + 2H_2O_{(l)}$ at $25\,^{\circ}C$ and $1\,atm$ pressure,$\Delta H = -874\,kJ.$ Then the change in internal energy $(\Delta E)$ is $...\,kJ$

In an isothermal expansion,the increase in volume with a decrease in pressure of a gas is greater than in an adiabatic expansion,because .............

Calculate the change in internal energy of the system if work done by the system is $18 \ J$ and absorbs heat $50 \ J$ in a particular reaction. (in $J$)

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