The P-V diagram of a system undergoing a ther | vedclass

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(D) Given,heat supplied to the system,$\Delta Q = 20 \, cal = 20 	imes 4.2 \, J = 84 \, J$.Work done on the system,$\Delta W = -50 \, J$ (Since work

Vedclass · Accepted Answer

$134$

Vedclass · Answer

(D) Given,heat supplied to the system,$\Delta Q = 20 \, cal = 20 	imes 4.2 \, J = 84 \, J$.Work done on the system,$\Delta W = -50 \, J$ (Since work is done on the system,it is negative).According to the first law of thermodynamics,$\Delta Q = \Delta U + \Delta W$,where $\Delta U$ is the change in internal energy.Therefore,$\Delta U = \Delta Q - \Delta W$.Substituting the values,$\Delta U = 84 \, J - (-50 \, J) = 84 \, J + 50 \, J = 134 \, J$.Thus,the change in internal energy between $A$ and $C$ is $134 \, J$.

The $P-V$ diagram of a system undergoing a thermodynamic transformation is shown in the figure. The work done on the system in going from $A \to B \to C$ is $50 \, J$ and $20 \, cal$ of heat is given to the system. The change in internal energy between $A$ and $C$ is ...... $J$.

Similar Questions

When $2 \ kg$ of water is boiled at atmospheric pressure,it converts into steam. The volume increases from $2 \times 10^{-3} \ m^3$ to $3.34 \ m^3$. The work done by the system is ....... $kJ$.

Write and explain the first law of thermodynamics.

$A$ gas absorbs $18 \ J$ of heat and work done on the gas is $12 \ J$. Then the change in internal energy of the gas is: (in $J$)

If $\Delta Q$ and $\Delta W$ represent the heat supplied to the system and the work done on the system respectively,then the first law of thermodynamics can be written as,where $\Delta U$ is the change in internal energy.

$Assertion:$ The heat supplied to a system is always equal to the increase in its internal energy.
$Reason:$ When a system changes from one thermal equilibrium to another,some heat is absorbed by it.

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