(D) For an insulated container,the process is adiabatic,so $q = 0$.According to the first law of thermodynamics,$\Delta E = q + W$.Since $q = 0$,$\Del

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(D) For an insulated container,the process is adiabatic,so $q = 0$.According to the first law of thermodynamics,$\Delta E = q + W$.Since $q = 0$,$\Delta E = W$.The work done $W$ against a constant external pressure is given by $W = -P_{ext} \Delta V$.$W = -10 \ atm \times (5.2 \ L - 4.2 \ L) = -10 \ atm \cdot L$.Since $1 \ atm \cdot L = 101.3 \ J$,then $W = -10 \times 101.3 \ J = -1013 \ J$.Therefore,$\Delta E = -1013 \ J$.

Class 11 Chemistry Thermodynamics First law of thermodynamics

Easy

$A$ gas is allowed to expand in an insulated container against a constant external pressure of $10 \ atm$ from an initial volume $4.2 \ L$ to $5.2 \ L$. The change in internal energy $\Delta E$ of the gas will be $:-$

A
$+1013 \ J$
B
$+10 \ atm \cdot L$
C
$-1013 \ atm \cdot L$
D
$-1013 \ J$

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Thermodynamics

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First law of thermodynamics

At the $1$ bar pressure,the volume of a gas is $0.6 \ L$. If the gas receives $122 \ J$ of heat at $1$ bar pressure,the volume becomes $2 \ L$. Calculate the change in its internal energy. $(1 \ L \cdot bar = 101.32 \ J)$

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For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the relationship between $\Delta H$ and $\Delta U$ is:

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In a process,$701 \, J$ of heat is absorbed by a system and $394 \, J$ of work is done by the system. What is the change in internal energy for the process (in $, J$)?

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In a cylinder,$1.0 \, \text{kcal}$ of heat is added to $1.2 \, \text{L}$ of $O_2$ gas at a constant pressure of $1 \, \text{atm}$. The volume changes to $1.5 \, \text{L}$. Calculate the change in internal energy $(\Delta U)$ for this process. (in $, \text{kcal}$)

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$A$ gas is allowed to expand in an insulated container against a constant external pressure of $10 \ atm$ from an initial volume $4.2 \ L$ to $5.2 \ L$. The change in internal energy $\Delta E$ of the gas will be $:-$

Similar Questions

At the $1$ bar pressure,the volume of a gas is $0.6 \ L$. If the gas receives $122 \ J$ of heat at $1$ bar pressure,the volume becomes $2 \ L$. Calculate the change in its internal energy. $(1 \ L \cdot bar = 101.32 \ J)$

For the reaction $C_3H_8(g) + 5O_2(g) \rightarrow 3CO_2(g) + 4H_2O(l)$,the value of $\Delta H - \Delta U$ is:

For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the relationship between $\Delta H$ and $\Delta U$ is:

In a process,$701 \, J$ of heat is absorbed by a system and $394 \, J$ of work is done by the system. What is the change in internal energy for the process (in $, J$)?

In a cylinder,$1.0 \, \text{kcal}$ of heat is added to $1.2 \, \text{L}$ of $O_2$ gas at a constant pressure of $1 \, \text{atm}$. The volume changes to $1.5 \, \text{L}$. Calculate the change in internal energy $(\Delta U)$ for this process. (in $, \text{kcal}$)

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