At a given temperature, k = 1.3 x 10-2 for the reaction:
N2(g) + 3H2(g) <--> 2NH3(g)
Calculate values of K for the following reactions at this temperature.
a.) 1/2N2(g) + 3/2H2(g) <--> NH3(g)
b.) 2NH3(g) <--> N2(g) + 3H2(g)
c.) NH3(g) <--> 1/2N2(g) + 3/2 H2(g)
d.) 2N2(g) + 6H2(g) <--> 4NH3(g)
a.) k =
b.) k =
c.) k =
d.) k =
For the reaction:
2NO(g) + 2H2(g) <--> N2(g) + 2H2O(g)
it is determined that, at equilibrium at a particular temperature, the concentrations are as follows:
[NO(g)] = 8.1 x 10-3 M
[H2(g)] = 4.1 x 10-5 M
[N2(g)] = 5.3 x 10-2 M
[H2O(g)] = 2.9 x 10-3 M
Calculate the value of K for the reaction at this temperature.
At a particular temperature, a 3.0L flask contains 2.4 mole of Cl2, 1.0 mol of NOCl, and 4.5 x 10-3 mole of NO. Calculate K at this temperature for the following reaction.
2NOCl(g) <--> 2NO(g) + Cl2(g)