The equilibrium constant- Kp for the reaction- 2NOCl-g- 2NO-g- - Cl2-g-is 6-95-10-8 at 298K- The standard Gibb-s free energy change- -G- at 298K will be -R-2calK-1mole-1- -log6-95-0-8420-a- 4-912 kcal -b- 14-74 kcal-c- 7-3 kcal-d- 9-825 kcal

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Potassium Dichromate

The equilibri...

Question

The equilibrium constant, Kp for the reaction, 2NOCl(g) <-----> 2NO(g) + Cl2(g) is 6.95*10^-8 at 298K. The standard Gibb's free energy change, ΔG° at 298K will be (R=2calK^-1mole^-1) (log6.95=0.8420) (a) 4.912 kcal (b) 14.74 kcal (c) 7.3 kcal (d) 9.825 kcal

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K_{p}

2 N O C l (g) ⇌ 2 N O (g) + C l_{2} (g)

0.95 \times 10^{- 6}

298 K

Δ G^{o}

298 K

(R = 2 c a l K^{- 1} m o l e^{- 1})

(log 6.95 = 0.8420)

K_{p}

10^{- 8}

Δ G^{⊖}

R = 2 c a l K^{- 1} m o l^{- 1})

△ G^{o} = - 115 k J a t 298 K .

K_{P}

l o g K_{P} . (R = 8.314 J K^{- 1} m o l^{- 1})

K_{p}

10^{- 3}

Δ G^{o}

27^{o} C

R = 2 c a l K^{- 1} {m o l}^{- 1}

2 N O C l (g) ⇌ 2 N O (g) + {C l}_{2} (g)

298 K

Δ H^{o}

Δ S^{o}

298 K

77.2 k J {m o l}^{- 1}

122 J K {m o l}^{- 1}

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