Write the equilibrium constant expression for each of the following reactions:
A. 4NO(g)+2O^2 <--> 2N^2O^4(g)
B. 2NO(g)+ Br^2(g) <--> 2NOBr(g)
C. CO(g)+ 2H^2(g) <--> CH^3OH(g)
D. SO^2(g) + NO^2(g) <--> SO^3(g) + NO(g)
What is your problem with these. Keq expressions are the same.
K = (products)^x/(reactants)^y and raise each substance to the power indicated by the coefficient.
you have to find the equilibrium constant for them.
No, the problem says to write the equilibrium constant expression. Nothing about finding the value of K.
Not the value, the equilibrium constant. DrBob222, there's no instance of the letter "K" except in your own statement
To write the equilibrium constant expressions, you need to remember the following rules:
1. Write the balanced equation for the reaction.
2. Exclude any pure solids or liquids from the expression.
3. Express the concentrations of gases in terms of partial pressure (P) or molar concentrations (C), depending on the given information.
Let's go through each reaction and write their equilibrium constant expressions:
A. 4NO(g) + 2O2(g) ⇌ 2N2O4(g)
The equilibrium constant expression, denoted as Kc or Kp (depending on whether concentrations or partial pressures are used), is given by:
Kc = [N2O4]^2 / ([NO]^4 * [O2]^2)
B. 2NO(g) + Br2(g) ⇌ 2NOBr(g)
The equilibrium constant expression is:
Kc = [NOBr]^2 / ([NO]^2 * [Br2])
C. CO(g) + 2H2(g) ⇌ CH3OH(g)
The equilibrium constant expression is:
Kc = [CH3OH] / ([CO] * [H2]^2)
D. SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)
The equilibrium constant expression is:
Kc = ([SO3] * [NO]) / ([SO2] * [NO2])
Please note that the equilibrium constant expressions are based on the balanced equations for these reactions.