It is possible to predict the equilibrium constant of a reaction by combining two or more reactions
Question:
It is possible to predict the equilibrium constant of a reaction by combining two or more reactions for which the value of K is known. When combining equilibrium constants, it is important to note the following:
When a reaction is reversed, its K value is inverted; that is, K reverse=1/ K forward.
When the coefficients of a reaction are multiplied by a factor, the K value is raised to the power of that factor.
When reactions are added, their K values are multiplied.
Part A
Determine the value of the equilibrium constant, K goal, for the reaction
N2(g)+H2O(g)⇌NO(g)+12N2H4(g), K goal=?
by making use of the following information:
1. N2(g)+O2(g)⇌2NO(g), | K 1 = | 4.10×10−31 |
2. N2(g)+2H2(g)⇌N2H4(g), | K 2 = | 7.40×10−26 |
3. 2H2O(g)⇌2H2(g)+O2(g), | K 3 = | 1.06×10−10 |
Part B
Determine the equilibrium constant, K goal, for the reaction
4PCl5(g)⇌P4(s)+10Cl2(g), K goal=?
by making use of the following information:
P4(s)+6Cl2(g)⇌4PCl3(g), K 1=2.00×1019
PCl5(g)⇌PCl3(g)+Cl2(g), K 2=1.13×10−2