(C) According to the first law of thermodynamics,the change in internal energy $(\Delta U)$ is given by: $\Delta U = q + w$. Here,the system absorbs h

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(C) According to the first law of thermodynamics,the change in internal energy $(\Delta U)$ is given by: $\Delta U = q + w$. Here,the system absorbs heat,so $q = +450 \ J$. The system performs work,so $w = -600 \ J$. Therefore,$\Delta U = 450 \ J - 600 \ J = -150 \ J$. Since $\Delta U = U_2 - U_1$,we have $U_2 - U_1 = -150 \ J$. Thus,the final internal energy $U_2 = U_1 - 150 \ J$.

Class 11 Chemistry Thermodynamics First law of thermodynamics

Medium

If the initial internal energy of a system is $U_1$,and it absorbs $450 \ J$ of heat from the surroundings and performs $600 \ J$ of work,what will be the final internal energy of the system?

A
$(U_1 + 150) \ J$
B
$(U_1 + 1050) \ J$
C
$(U_1 - 150) \ J$
D
None of these

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First law of thermodynamics

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If the initial internal energy of a system is $U_1$,and it absorbs $450 \ J$ of heat from the surroundings and performs $600 \ J$ of work,what will be the final internal energy of the system?

Similar Questions

If $2 \text{ mole}$ of an ideal gas expand isothermally and reversibly at $27^{\circ}C$ from $1 \text{ dm}^3$ to $1 \text{ m}^3$, calculate the work done. [$R = 8.314 \text{ J K}^{-1} \text{mol}^{-1}$] (in $\text{ kJ}$)

What is the final temperature of $0.10 \ mol$ monoatomic ideal gas that performs $75 \ cal$ of work adiabatically if the initial temperature is $227 \ ^\circ C$? (Use $R = 2 \ cal \cdot K^{-1} \cdot mol^{-1}$)

When $x \ kJ$ heat is provided to a system,work equivalent to $y \ J$ is done on it. What is the internal energy change during this operation?

$A$ gas expands isothermally against a constant external pressure of $1 \ bar$ from $10 \ dm^3$ to $20 \ dm^3$ by absorbing $800 \ J$ of heat from the surroundings. Calculate the value of $\Delta U$. (in $J$)

$A$ mixture of $2 \ mol$ of $CO_{(g)}$ and $1 \ mol$ of $O_{2(g)}$ is ignited to convert $CO$ to $CO_2$. Which of the following relations is correct?

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