Part A What is the numerical value of Kc for the following reaction if the equilibrium mixture contains 0.51 M C3H6O, 0.30 M O2, 1.8 M CO2, and 2.0 M H2O? C3H6O(g)+4O2(g)⇌3CO2(g)+3H2O(g)
A) 2.4 × 101B) 1.1 × 104C) 8.9 × 10-5D) 4.3 × 10-2

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as [tex]K_c[/tex].

The given balanced equilibrium reaction is,

[tex]C_3H_6O(g)+4O_2(g)\rightleftharpoons 3CO_2(g)+3H_2O(g)[/tex]

At eqm. conc. (0.51) M (0.30) M (1.8) M (2.0)M

The expression for equilibrium constant for this reaction will be,

[tex]K_c=\frac{[CO_2]^3\times [H_2O]^3}{[O_2]^4\times [C_3H_6O]^1}[/tex]

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

[tex]K_c=\frac{(1.8)^3\times (2.0)^3}{(0.30)^4\times (0.51)^1}[/tex]

[tex]K_c=1.1\times 10^4[/tex]

Thus the value of the equilibrium constant is [tex]1.1\times 10^4[/tex]

Part A What is the numerical value of Kc for the following reaction if the equilibrium mixture contains 0.51 M C3H6O, 0.30 M O2, 1.8 M CO2, and 2.0 M H2O? C3H6O(g)+4O2(g)⇌3CO2(g)+3H2O(g) A) 2.4 × 101B) 1.1 × 104C) 8.9 × 10-5D) 4.3 × 10-2

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Part A What is the numerical value of Kc for the following reaction if the equilibrium mixture contains 0.51 M C3H6O, 0.30 M O2, 1.8 M CO2, and 2.0 M H2O? C3H6O(g)+4O2(g)⇌3CO2(g)+3H2O(g)
A) 2.4 × 101B) 1.1 × 104C) 8.9 × 10-5D) 4.3 × 10-2