The work done to increase the volume of $2$ moles of an ideal gas from $V$ to $2V$ at a constant temperature $T$ is $W$. The work to be done to increase the volume of $2$ moles of the same gas from $2V$ to $4V$ at the same constant temperature $T$ is:
- A$0.5 W$
- B$W$
- C$2 W$
- D$4 W$
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Work done by a system under isothermal change from a volume $V_1$ to $V_2$ for a gas which obeys Van der Waals' equation $(V - n\beta) \left( P + \frac{\alpha n^2}{V^2} \right) = nRT$.
Difficult
View SolutionDuring an isothermal expansion,a confined ideal gas does $-150 \, J$ of work against its surroundings. This implies that
An ideal gas is subjected to an isothermal expansion such that its volume changes from $V_i$ to $V_f$ and pressure from $P_i$ to $P_f$. The work done on the gas is:
In an isothermal process,which statement is wrong?
Easy
View Solution$Assertion :$ The isothermal curves intersect each other at a certain point.
$Reason :$ The isothermal changes take place rapidly,so the isothermal curves have very little slope.
$Reason :$ The isothermal changes take place rapidly,so the isothermal curves have very little slope.
Medium
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