(A) The container is insulated,which means no heat exchange occurs with the surroundings. Therefore,the process is adiabatic,so $q = 0$.According to t

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(A) The container is insulated,which means no heat exchange occurs with the surroundings. Therefore,the process is adiabatic,so $q = 0$.According to the first law of thermodynamics,$\Delta U = q + W$.Since $q = 0$,we have $\Delta U = W$.Stirring the liquid with a paddle performs work on the system,so $W \neq 0$,which consequently leads to $\Delta U \neq 0$.

Class 11 Chemistry Thermodynamics First law of thermodynamics

Medium

In a closed insulated container,a liquid is stirred with a paddle to increase its temperature. Which of the following is correct?

A
$\Delta U = W \neq 0, q = 0$
B
$\Delta U = W = q \neq 0$
C
$\Delta U = 0, W = q \neq 0$
D
$W = 0, \Delta U = q \neq 0$

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Thermodynamics

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First law of thermodynamics

$A$ gas expands isothermally from $10 \, dm^3$ to $20 \, dm^3$ at a constant external pressure of $1 \, atm$. If it absorbs $800 \, J$ of heat from the surroundings,what is the value of $\Delta U$ in $J$ for this process?

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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

Medium

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If $3 \ mol$ of an ideal gas at $300 \ K$ expand isothermally from $30 \ dm^3$ to $45 \ dm^3$ against a constant opposing pressure of $80 \ kPa$,then the amount of heat transferred is . . . . . . $J$.

DifficultJEE MAIN 2024

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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?

DifficultMHT CET 2021

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Which among the following reactions exhibits $\Delta H = \Delta U$?

MediumMHT CET 2023

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In a closed insulated container,a liquid is stirred with a paddle to increase its temperature. Which of the following is correct?

Similar Questions

$A$ gas expands isothermally from $10 \, dm^3$ to $20 \, dm^3$ at a constant external pressure of $1 \, atm$. If it absorbs $800 \, J$ of heat from the surroundings,what is the value of $\Delta U$ in $J$ for this process?

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

If $3 \ mol$ of an ideal gas at $300 \ K$ expand isothermally from $30 \ dm^3$ to $45 \ dm^3$ against a constant opposing pressure of $80 \ kPa$,then the amount of heat transferred is . . . . . . $J$.

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?

Which among the following reactions exhibits $\Delta H = \Delta U$?

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