# Question #edf1e

##### 2 Answers

#### Answer:

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

#### Answer:

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).