The following reaction mixture contains 0.22 M CH4, 0.67 M CO2 and 1.3 M H2O. Which of the following statements is TRUE concerning this system?
4 CuO(s) + CH4(g) ? CO2(g) + 4 Cu(s) + 2 H2O(g)
Kc = 1.10
a)the reaction is running fastest toward the reactants
b)the reaction is running fastest toward the products
c)the value of the equilibrium constant will increase
d)the value of the reaction quotient will increase
e)the reaction is at equilibrium

Reaction is shifting left toward reactant side

Explanation:

4CuO(s) + CH₄(g) <=?=> CO₂(g) + Cu(s) + 2H₂O(g)

     0.22M             0.67M        1.30M

Qc = [O₂(g)][H₂O(l)]²/[CH₄(g)] = (0.67)(1.30)²/(0.22) =5.12

Kc = 1.1 < Qc = 5.12 => Reaction is shifting LEFT and reactant concentrations are increasing with product concentrations decreasing. Qc will be decreasing and final Kc value will be lower than original Qc upon reaching equilibrium stability.  

FYI Note => For reaction mixtures the following is a good guide to reaction response to applied system stress. Note the conclusion follows the direction the inequality symbol is pointing.  

Kc  <  Qc  => Rxn system is shifting Left

Kc =   Qc  => Rxn system is at equilibrium

Kc >  Qc  => Rxn system is shifting Right

chemical properties are the characteristic of matter which can only be observed by changing the chemical identity of a sample like flammability reactivity and toxicity.

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.