The concentration equilibrium constant for the gas-phase reaction H2 CO ⇌H2+CO has the numerical

step 1 On the balanced equation, H2 -7 gives out H2 plus 0. It gives out K -J equals to 0 .5 and the re

The concentration equilibrium constant for the gas-phase...

The concentration equilibrium constant for the gas-phase reaction $$\mathrm{H}_{2} \mathrm{CO} \rightleftharpoons \mathrm{H}_{2}+\mathrm{CO}$$ has the numerical value 0.50 at a given temperature. A mixture of $\mathrm{H}_{2} \mathrm{CO}, \mathrm{H}_{2},$ and $\mathrm{CO}$ is introduced into a flask at this temperature. After a short time, analysis of a small sample of the reaction mixture shows the concentrations to be $\left[\mathrm{H}_{2} \mathrm{CO}\right]=0.50 \mathrm{M},\left[\mathrm{H}_{2}\right]=0.80 \mathrm{M},$ and $[\mathrm{CO}]=0.25 \mathrm{M}$ Classify each of the following statements about this reaction mixture as true or false. (a) The reaction mixture is at equilibrium. (b) The reaction mixture is not at equilibrium, but no further reaction will occur. (c) The reaction mixture is not at equilibrium, but will move toward equilibrium by using up more $\mathrm{H}_{2} \mathrm{CO}$. (d) The forward rate of this reaction is the same as the reverse rate.

The concentration equilibrium constant for the gas-phase reaction
$$\mathrm{H}_{2} \mathrm{CO} \rightleftharpoons \mathrm{H}_{2}+\mathrm{CO}$$
has the numerical value 0.50 at a given temperature. A mixture of $\mathrm{H}_{2} \mathrm{CO}, \mathrm{H}_{2},$ and $\mathrm{CO}$ is introduced into a flask at this temperature. After a short time, analysis of a small sample of the reaction mixture shows the concentrations to be $\left[\mathrm{H}_{2} \mathrm{CO}\right]=0.50 \mathrm{M},\left[\mathrm{H}_{2}\right]=0.80 \mathrm{M},$ and $[\mathrm{CO}]=0.25 \mathrm{M}$ Classify each of the following statements about this reaction mixture as true or false.
(a) The reaction mixture is at equilibrium.
(b) The reaction mixture is not at equilibrium, but no further reaction will occur.
(c) The reaction mixture is not at equilibrium, but will move toward equilibrium by using up more $\mathrm{H}_{2} \mathrm{CO}$.
(d) The forward rate of this reaction is the same as the reverse rate.

Key Concepts

Chemical Equilibrium

Chemical equilibrium is the state in a chemical reaction where the rate of the forward reaction equals the rate of the reverse reaction, leading to constant concentrations of reactants and products over time. Even though the individual reactions continue to occur, there is no net change in the composition of the system. This concept is fundamental in understanding how reactions behave under various conditions and how they can be influenced by changes in concentration, temperature, and pressure.

Equilibrium Constant (Kc)

The equilibrium constant (Kc) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium, with each concentration raised to the power of its stoichiometric coefficient. This constant provides insight into the position of equilibrium, indicating whether the reaction favors the formation of products or reactants under specific conditions.

Reaction Quotient (Q)

The reaction quotient (Q) is calculated using the same expression as the equilibrium constant but with the actual, potentially non-equilibrium, concentrations of the reactants and products. Comparing Q to the equilibrium constant (Kc) allows one to predict the direction in which a reaction mixture will proceed to achieve equilibrium.

Dynamic Equilibrium

Dynamic equilibrium refers to the condition in a reversible reaction where the forward and reverse reaction rates are equal, resulting in no further change in the concentrations of reactants and products. This concept highlights that even though the system appears static, molecular processes continue to occur in both directions at equal rates.

Reaction Kinetics

Reaction kinetics deals with the rates at which chemical reactions occur and the factors that influence these rates. In the context of equilibrium, it explains that when a system reaches equilibrium, the individual forward and reverse reactions continue to occur at the same rate, ensuring the overall concentration of substances in the system remains constant.

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