Which of the following statements regarding the first law of thermodynamics is correct?
- AThe energy of the isolated system plus the energy of the surrounding is constant.
- BThe energy of the isolated system minus the energy of the surrounding is constant.
- CThe energy of an isolated system is constant.
- DThe energy of an isolated system varies.
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Assertion : For an isothermal reversible process $Q = -W$,i.e.,work done by the system equals the heat absorbed by the system.
Reason : Enthalpy change $(\Delta H)$ is zero for an isothermal process.
Reason : Enthalpy change $(\Delta H)$ is zero for an isothermal process.
MediumAIIMS 2011
View SolutionIf a system absorbs $30 \ kJ$ of heat and performs $12 \ kJ$ of work on the surroundings,what is the increase in internal energy of the system (in $kJ$)?
$A$ gas expands from a volume of $4 \ L$ to $14 \ L$ against a constant external pressure of $1 \ atm$ in a cylinder with a frictionless piston. During this process,the gas absorbs $800 \ J$ of heat from the surroundings. Calculate the change in internal energy $\Delta E$ in $J$. (in $.7$)
Medium
View Solution$A$ 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?
Difficult
View SolutionWhat is the change in internal energy if a system gains $x \ J$ of heat and $y \ J$ of work is done on it?
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