The value of $$\log_{10} K$$ for a reaction $$A \rightleftharpoons B$$ is
(Given : $$\triangle_rH_{298K}^{\circ}$$ = -54.07 kJ mol$$^{-1}$$, $$\triangle_rS_{298K}^{\circ}$$ = 10 JK$$^{-1}$$ mol$$^{-1}$$ and R = 8.314 JK$$^{-1}$$ mol$$^{-1}$$; $$2.303 \times 8.314 \times 298 = 5705$$)

A

5

B

10

C

95

D

100