Question #edf1e
2 Answers
I assume you are looking for the final equilibrium concentrations of this reaction.
Explanation:
First, you must balance the chemical equation in order to get the coefficients needed for the rate reaction:
#2N_2 + O_2 rightleftharpoons 2N_2O#
Then you need to set up an ICE (Initial, Change, Equilibrium) chart to find the factors that need to be solved in the equation for a numerical result:
The volume is irrelevant as long as the molar quantities are known and it is a gas mixture. It is only necessary if you are given solution volumes and need to correct from the standard moles/Liter to actual moles in solution for liquid solutions.
#" " " "2N_2" " " " + " " " "O_2" " rightleftharpoons " " " "2N_2O#
(this is why you need to balance the equation, not all of the
The equilibrium equation is
#K_c = (["Products"]^A)/(["Reactants"]^B)" "# , where
The equation for this system at equilibrium is thus:
Substituting the problem values from the ICE chart:
Solve for
Also asked: Is this also how to calculate composition of equilibrium?
YES.
Explanation:
In general, the steps to determine the composition of an equilibrium mixture, given the chemical reaction equation, starting concentrations of the reactants, and the equilibrium constant are the same.
- Write out the balanced chemical reaction.
- Set up the I.C.E table to determine the equilibrium concentrations of each species.
- Use the values from the Equilibrium line of the ICE (including the unknown factors) to set up the equilibrium equation with the equilibrium constant.
- Solve the equation for the unknown quantity, then back-calculate any other species that may depend on that value (if necessary).