One mole each of He and A(g) are taken in a 10 L closed flask and heated to 400 K to establish the following equilibrium.
A(g) $$\rightleftharpoons$$ B(g)
K$$_c$$ for this reaction at 400 K is 4.0. The partial pressures (in atm) of He and B(g) are respectively (at equilibrium)
(Assume He, A(g) and B(g) behave as ideal gases)
(Given: R = 0.082 L atm K$$^{-1}$$ mol$$^{-1}$$)

A

3.28, 2.624

B

2.624, 3.28

C

3.28, 0.656

D

0.656, 6.56