Question

Two equilibrium reactions of nitrogen with oxygen, with their corresponding equilibrium constants (kc) at a certain temperature, are given below. What are the equilibrium reactions and their equilibrium constants?

Answer 1

Two chemical equilibrium reactions involving nitrogen are N2 + 3H2 = 2NH3 with Kc of 6.00 × 10^-2 and N2 + O2 = 2NO with Kc of 4.1 × 10^-4 at 2000 °C. Calculations of equilibrium concentrations depend on these constants and initial concentrations of reactants.

Step-by-step explanation:

The equilibrium reactions of nitrogen with oxygen and their corresponding equilibrium constants (Kc) are important in understanding chemical equilibrium. Two reactions are commonly studied:

1. The reaction of nitrogen (N2) and hydrogen (H2) to produce ammonia (NH3), which at a certain temperature has a Kc of 6.00 × 10-2.
2. The reaction of nitrogen (N2) with oxygen (O2) to form nitrogen monoxide (NO), which at 2000 °C has a Kc of 4.1 × 10-4.

For instance, to calculate the equilibrium concentration of ammonia, if the equilibrium concentrations of nitrogen and hydrogen are 4.26 M and 2.09 M respectively, we apply the equilibrium constant for the reaction N2(g) + 3H2(g) = 2NH3(g).

Another example is determining the equilibrium concentration of nitrogen monoxide (NO) in air at 1 atm pressure and 2000 °C when the equilibrium concentrations of N2 and O2 are 0.036 M and 0.0089 M, respectively.