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Readme [11.4K]
3 years ago
11

Use the reactions below and their equilibrium constants to predict the equilibrium constant for the reaction 2A(s)⇌3D(g). A(s) ⇌

12 B(g)+C(g), K1=0.0334 3D(g) ⇌ B(g)+2C(g), K2=2.35
Chemistry
1 answer:
Liula [17]3 years ago
7 0

Answer : The equilibrium constant for the reaction will be, 4.747\times 10^{-4}

Explanation :

The following equilibrium reactions are :

(1) A(s)\rightleftharpoons \frac{1}{2}B(g)+C(g)           K_1=0.0334

(2) 3D(g)\rightleftharpoons B(g)+2C(g)          K_2=2.35  

The final equilibrium reaction is :

2A(s)\rightleftharpoons 3D(g)         K_{eqm}=?

Now we have to calculate the value of K_{eqm} for the final reaction.

First we have to multiply equation (1) by 2 that means we are taking square of equilibrium constant 1 and reverse the equation 2 that means we are dividing equilibrium constant 2, we get the final equilibrium reaction and the expression of final equilibrium constant is:

K_{eqm}=\frac{(K_1)^2}{K_2}

Now put all the given values in this expression, we get :

K_{eqm}=\frac{(0.0334)^2}{2.35}

K_{eqm}=4.747\times 10^{-4}

Therefore, the value of K_{eqm} for the final reaction is, 4.747\times 10^{-4}

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