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Semmy [17]
3 years ago
12

Determine the value of the equilibrium constant, KgoalKgoalK_goal, for the reaction CO2(g)⇌C(s)+O2(g)CO2(g)⇌C(s)+O2(g), Kgoal=?

Kgoal=? by making use of the following information: 1. 2CO2(g)+2H2O(l)⇌CH3COOH(l)+2O2(g)2CO2(g)+2H2O(l)⇌CH3COOH(l)+2O2(g), K1 = K1 = 5.40×10−165.40×10−16 2. 2H2(g)+O2(g)⇌2H2O(l)2H2(g)+O2(g)⇌2H2O(l), K2 = K2 = 1.06×10101.06×1010 3. CH3COOH(l)⇌2C(s)+2H2(g)+O2(g)CH3COOH(l)⇌2C(s)+2H2(g)+O2(g), K3 = K3 = 2.68×10−92.68×10−9
Chemistry
1 answer:
NISA [10]3 years ago
4 0

Answer:

The value of the equilibrium constant for reaction asked is 1.24\times 10^{-7}.

Explanation:

CO_2(g)\rightleftharpoons C(s)+O_2(g)

K_{goal}=?

K_{goal}=\frac{[C][O_2]}{[CO_2]}

2CO_2(g)+2H_2O(l)\rightleftharpoons CH_3COOH(l)+2O_2(g)..[1]

K_1=\frac{[CH_3COOH][O_2]^2}{[CO_2]^2[H_2O]^2}

2H_2(g)+O2(g)\rightleftharpoons 2H_2O(l)..[2]

K_2=\frac{[H_2O]^2}{[H_2]^2[O_2]}

CH_3COOH(l)\rightleftharpoons 2C(s)+2H_2(g)+O_2(g)..[3]

K_3=\frac{[C]^2[H_2]^2[O_2]}{[CH_3COOH]}

[1] +  [2] + [3]

2CO_2(g)\rightleftharpoons 2C(s)+2O_2(g)

 ( on adding the equilibrium constant will get multiplied with each other)

K=K_1\times K_2\times K_3

K=5.40\times 10^{-16}\times 1.06\times 10^{10}\times 2.68\times 10^{-9}

K=1.53\times 10^{-14}

K=\frac{[C]^2[O_2]^2}{[CO_2]^2}

On comparing the K and K_{goal}:

K^2=K_{goal}

K_{goal}=\sqrt{K}=\sqrt{1.53\times 10^{-14}}=1.24\times 10^{-7}

The value of the equilibrium constant for reaction asked is 1.24\times 10^{-7}.

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Answer:

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Explanation:

Hello!

In this case, since we have the amount of molecules of this this compound, we are able to compute the moles out there by using the Avogadro's number:

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