At constant volume, 6.0 mol of $$H_2$$ gas at $$0^\circ C$$ and 100 kPa was heated to 250 kPa. The molar heat capacity of $$H_2$$ at constant pressure $$(C_P) = 28.9$$ $$\text{J mol}^{-1} \text{K}^{-1}$$ (assume that the heat capacity values do not change with temperature). The final temperature of the $$H_2$$ gas and the change in entropy of the process are

A

$$273^\circ C$$ and 113 $$\text{kJ mol}^{-1} \text{K}^{-1}$$

B

$$410^\circ C$$ and 158.8 $$\text{J mol}^{-1} \text{K}^{-1}$$

C

$$682.5^\circ C$$ and 113 $$\text{J mol}^{-1} \text{K}^{-1}$$

D

682.5 K and 113 $$\text{J mol}^{-1} \text{K}^{-1}$$