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Chemistry Question on Equilibrium Constant

The value of KcK_c for the reaction : A+3B⇌2C{A + 3B\rightleftharpoons2C} at 400∘C400^\circ C is 0.5.0.5. Calculate the value of KPK_P

A

1.64×10−41.64 \times 10^{-4}

B

1.64×10−61.64 \times 10^{-6}

C

1.64×10−51.64 \times 10^{-5}

D

1.64×10−31.64 \times 10^{-3}

Answer

1.64×10−41.64 \times 10^{-4}

Explanation

Solution

Kp=Kc[RT]gΔn Δn=2−4=−2K_{p}=K_{c}\left[RT\right]^{\Delta n}_{g}\,\Delta n=2-4=-2
T=673K,Kc=0.5,T=673K, K_{c}=0.5,
R=0.082 L. atm. mol−1 K−1R=0.082\,L.\,atm.\,mol^{-1}\,K^{-1}
Kp=0.5×(0.082×673)−2=1.64×10−4 atm.K_{p}=0.5\times\left(0.082\times673\right)^{-2} =1.64\times10^{-4}\,atm.