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Standard XII

Chemistry

Solubility Product

Calculate K...

Question

Calculate $K_{p}$ for the reaction,
$C (s) + H_{2} O_{(g)} ⇌ C O_{(g)} + H_{2 (g)}$ at 990 K if the equilibrium concentration are as follows :
$[H_{2} O] = 1.10 M, [C O] = [H_{2}] = 0.2 M, R = 0.08206 L a t m k^{- 1} m o l^{- 1}$

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Solution

First calculate $K_{c}$ ( $K_{p}$ =2.954)

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Q. The value of

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Q. The value of Kc = 4.24 at 800 Kfor the reaction CO(g) + H2O (g) gives rise to CO2(g) + H2(g) Calculate equilibrium concentrations of CO2, H2, CO and H2O at 800 K , if only CO and H2O are present initially at concentration of 0.10 M each ?

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Calculate Kp for the reaction, C(s)+H2O(g)⇌CO(g)+H2(g) at 990 K if the equilibrium concentration are as follows :[H2O]=1.10M,[CO]=[H2]=0.2M,R=0.08206Latmk−1mol−1

First calculate Kc (Kp=2.954)

Calculate $K_{p}$ for the reaction,
$C (s) + H_{2} O_{(g)} ⇌ C O_{(g)} + H_{2 (g)}$ at 990 K if the equilibrium concentration are as follows :
$[H_{2} O] = 1.10 M, [C O] = [H_{2}] = 0.2 M, R = 0.08206 L a t m k^{- 1} m o l^{- 1}$

First calculate $K_{c}$ ( $K_{p}$ =2.954)