For an ideal gas
a)   The change in internal energy in a constant- pressure process from temperature $T_{1}$ to $T_{2}$ is equal to $n C_{v} (T_{2} - T_{1})$ , where $C_{v}$ is the molar heat capacity at constant volume and n is the number of moles of the gas
b)   The change in internal energy of the gas and the work done by the gas are equal in magnitude in an adiabatic process
c)   The internal energy does not change in an isothermal process
d)   No heat is added or removed in an adiabatic process

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only a, b are correct

all are correct

only c, d are correct

only b, d are correct

answer is D.

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Detailed Solution

For any process $∆ U = n C_{v} d T$ and $C_{v} = f \frac{R}{2}$

For adiabatic process Q = 0

hence from first law. $∆ U =$ -W

So both have same magnitude.

In isothermal process internal energy is constant.

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