With increase in temperature, the value of $$K$$ for exothermic reaction decreases because the entropy change of the system is positive

With increase in temperature, the value of $$K.$$ for endothermic reaction increases because unfavorable change in entropy of the surroundings decreases

With increase in temperature, the value of $$K$$ for endothermic reaction increases because the entropy change of the system is negative

with increase in temperature, the value of $$K$$ for exothermic reaction decreases because favorable change in entropy of the surroundings decreases

The work done on the gas is maximum when it is compressed irreversibly from $$\left( {{p_2},{V_2}} \right)$$ to $$\left( {{p_1},{V_1}} \right)$$ against constant pressure $${p_1}$$

If the expansion is carried out freely, it is simultaneously both isothermal as well as adiabatic

The work done by the gas is less when it is expanded reversibly from $${V_1}$$ to $${V_2}$$ under adiabatic conditions as compared to that when expanded reverseibly from $${V_1}$$ to $${V_2}$$ under isothermal conditions

The change in internal energy of the gas is (i) zero, if it is expanded reversibly with $${T_1} = {T_2}$$ , and (ii) positive, if it is expanded reversibly under adiabatic conditions with $${T_1}\, \ne \,{T_2}$$

$$\Delta G$$ is positive

$$\Delta S_{system}$$ is positive

$$\Delta S_{surroundings}$$ = 0

$$\Delta H$$ = 0

T₁ = T₂

T₃ > T₁

w_isothermal > w_adiabatic

$$\Delta$$U_isothermal > $$\Delta$$U_adiabatic