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PSYCHO15rus [73]
3 years ago
11

Use the "x is small" approximation to find the concentration of the products in the following reaction which initially contains

only 0.85 M HCN. Decide whether using the approximation was valid or invalid.HCN(aq) ⇌ H+(aq) + CN−(aq), Kc= 6.17 x 10−10
Chemistry
1 answer:
Mrrafil [7]3 years ago
4 0

Answer:

Concentration of product at equilibrium ;

[H^+]=0.0000229 M

[CN^-]=0.0000229 M

Explanation:

HCN(aq)\rightleftharpoons H^+(aq) + CN^-(aq)

initially

0.85 M        0    0

(0.85-x)M    x      x

The equilibrium constant of reaction = K_c= 6.17\times 10^{-10}

The expression of an equilibrium cannot can be written as:

K_c=\frac{[H^+][CN^-]}{[HCN]}

6.17\times 10^{-10}=\frac{x\times x}{(0.85-x)}

Solving for x:

x = 0.0000229

Concentration of product at equilibrium ;

[H^+]=0.0000229 M

[CN^-]=0.0000229 M

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