(D) The container is thermally insulated,so there is no heat exchange with the surroundings,meaning $q = 0$. Work is done on the system by the mechani

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(D) The container is thermally insulated,so there is no heat exchange with the surroundings,meaning $q = 0$. Work is done on the system by the mechanical stirrer,so by the sign convention,$w > 0$. According to the first law of thermodynamics,$\Delta U = q + w$. Since $q = 0$ and $w > 0$,it follows that $\Delta U = w > 0$. Therefore,the internal energy of the system increases.

Class 11 Chemistry Thermodynamics First law of thermodynamics

Medium

$A$ sample of liquid in a thermally insulated container (a calorimeter) is stirred for $2 \ hr$ by a mechanical linkage to a motor in the surroundings. For this process:

A
$w < 0; q = 0; \Delta U = 0$
B
$w > 0; q > 0; \Delta U > 0$
C
$w < 0; q > 0; \Delta U = 0$
D
$w > 0; q = 0; \Delta U > 0$

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Class 11

Chemistry Questions

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Thermodynamics

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First law of thermodynamics

When a certain volume of gas expands against a constant external pressure of $2.40 \times 10^5 \ Pa$ at $300 \ K$ to a final volume of $2.2 \times 10^{-3} \ m^3$. If the work obtained is $-0.048 \ kJ$,what is the initial volume of the gas?

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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 $(C_v = 20\, J/K)$ .....$K$

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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:

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Assuming all reactions occur in an open vessel,for which reaction will $\Delta H = \Delta U$?

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$A$ system receives $100 \ cal$ of heat,and at the same time,$50 \ cal$ of work is done by the system. Calculate the change in internal energy. (in $cal$)

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$A$ sample of liquid in a thermally insulated container (a calorimeter) is stirred for $2 \ hr$ by a mechanical linkage to a motor in the surroundings. For this process:

Similar Questions

When a certain volume of gas expands against a constant external pressure of $2.40 \times 10^5 \ Pa$ at $300 \ K$ to a final volume of $2.2 \times 10^{-3} \ m^3$. If the work obtained is $-0.048 \ kJ$,what is the initial volume of the gas?

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 $(C_v = 20\, J/K)$ .....$K$

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:

Assuming all reactions occur in an open vessel,for which reaction will $\Delta H = \Delta U$?

$A$ system receives $100 \ cal$ of heat,and at the same time,$50 \ cal$ of work is done by the system. Calculate the change in internal energy. (in $cal$)

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