(B) For a process at constant volume,the work done $w = P \Delta V = 0$. According to the first law of thermodynamics,$\Delta U = q + w$. Since $w = 0

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$q = \Delta U = 500 \, J, w = 0$

(B) For a process at constant volume,the work done $w = P \Delta V = 0$. According to the first law of thermodynamics,$\Delta U = q + w$. Since $w = 0$,we have $\Delta U = q$. Given that the heat supplied $q = 500 \, J$,therefore $\Delta U = 500 \, J$ and $w = 0$.

Class 11 Chemistry Thermodynamics First law of thermodynamics

Medium

When $1 \, \text{mol}$ of a gas is heated at constant volume,the temperature increases from $298 \, K$ to $308 \, K$. If the heat supplied to the gas is $500 \, J$,which of the following statements is correct?

A
$q = w = 500 \, J, \Delta U = 0$
B
$q = \Delta U = 500 \, J, w = 0$
C
$q = w = 500 \, J, \Delta U = 0$
D
$\Delta U = 0, q = w = -500 \, J$

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Thermodynamics

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First law of thermodynamics

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When $1 \, \text{mol}$ of a gas is heated at constant volume,the temperature increases from $298 \, K$ to $308 \, K$. If the heat supplied to the gas is $500 \, J$,which of the following statements is correct?

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Calculate the change in internal energy of the system if $20 \ kJ$ work is done on the system and it releases $10 \ kJ$ heat in a particular reaction. (in $kJ$)

The heat change for the following reaction at $298 \ K$ and at constant pressure is $+7.3 \ kcal$: $A_2B_{(s)} \to 2A_{(s)} + 1/2B_{2(g)}$,$\Delta H = +7.3 \ kcal$. The heat change at constant volume would be:

For the reaction $C_2H_5OH_{(l)} + 3O_{2(g)} \rightarrow 2CO_{2(g)} + 3H_2O_{(l)}$,the enthalpy change $(\Delta H)$ at $27\,^oC$ is $-1366.5 \,kJ\,mol^{-1}$. What will be the value of the internal energy change $(\Delta U)$ in $kJ\,mol^{-1}$ at the same temperature?

For combustion of one mole of magnesium in an open container at $300 \ K$ and $1 \ bar$ pressure,$\Delta_{C}H^{\ominus} = -601.70 \ kJ \ mol^{-1}$,the magnitude of change in internal energy for the reaction is $.... \ kJ$. (Nearest integer)(Given : $R = 8.3 \ J \ K^{-1} \ mol^{-1}$ )

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For combustion of one mole of magnesium in an open container at $300 \ K$ and $1 \ bar$ pressure,$\Delta_{C}H^{\ominus} = -601.70 \ kJ \ mol^{-1}$,the magnitude of change in internal energy for the reaction is $.... \ kJ$. (Nearest integer)
(Given : $R = 8.3 \ J \ K^{-1} \ mol^{-1}$ )