What is the equilibrium constant in the following reaction

[C][O2]/[CO2]

[CO2]/[C][O2]

[C]^2[O2]^2/[CO2]^2

[CO2]^2/[C]^2[O2]^2

[CO2] / [C][02]

Anonymous is correct

The equilibrium constant in the following reaction can be determined by looking at the ratio of the products to the reactants with each species raised to the power of its stoichiometric coefficient.

The correct expression for the equilibrium constant is [CO2]^2/[C]^2[O2]^2.

The equilibrium constant, denoted as K, is a measure of the extent to which a chemical reaction reaches equilibrium. It provides information about the relative concentrations of reactants and products in the equilibrium state.

In the given reactions:

1. [C][O2]/[CO2]: This is the ratio of the concentration of C multiplied by the concentration of O2 to the concentration of CO2. However, without specific numerical values for the concentrations, it is not possible to determine the equilibrium constant from this ratio.

2. [CO2]/[C][O2]: This is the ratio of the concentration of CO2 to the product of the concentrations of C and O2. As with the first ratio, without actual concentration values, the equilibrium constant cannot be determined.

3. [C]^2[O2]^2/[CO2]^2: This is the ratio of the squared concentration of C multiplied by the squared concentration of O2 to the squared concentration of CO2. Similarly, without actual concentration values, the equilibrium constant cannot be determined from this ratio.

4. [CO2]^2/[C]^2[O2]^2: This ratio is the squared concentration of CO2 divided by the product of the squared concentrations of C and O2. Again, without specific concentration values, the equilibrium constant cannot be determined.

To find the equilibrium constant, you would need either the actual numerical values of the concentrations of reactants and products at equilibrium or the equilibrium expression and its corresponding balanced equation.