One mole of an ideal monoatomic gas is heated at a constant pressure of one atmosphere from ${0^o}C$ to ${100^o}C$. Then the change in the internal energy is
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(c) Change in internal energy is always equal to the heat supplied at constant volume.
i.e. $\Delta U = {(\Delta Q)_V} = \mu {C_V}\Delta T.$
For monoatomic gas ${C_V} = \frac{3}{2}R$
==> $\Delta U = \mu \,\left( {\frac{3}{2}R} \right)\Delta T = 1 \times \frac{3}{2} \times 8.31 \times (100 - 0)$
$ = 12.48 \times {10^2}J$
i.e. $\Delta U = {(\Delta Q)_V} = \mu {C_V}\Delta T.$
For monoatomic gas ${C_V} = \frac{3}{2}R$
==> $\Delta U = \mu \,\left( {\frac{3}{2}R} \right)\Delta T = 1 \times \frac{3}{2} \times 8.31 \times (100 - 0)$
$ = 12.48 \times {10^2}J$
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