I have gotten the equilibrium concentrations of N202 to be 2M and N02 to be 2M also.
After equilibirum is reached, a pistons is used to decrease the flask volume to 3L. Once equilibrium is established find the concentration and moles of each gas.
K = 2
How would I set up my ice chart? Do i double the concentrations at eq1 and use it as my initial?
Since you are increasing the pressure do you reverse the reaction? Please help idont know what to do.
I am uncertain of the reaction you are using.
The reaction is N204 <---> 2NO2. First equilibrium is set up and the [] Of both is 2M.
Now the pressure decreases the falsh volume to 3L. What will be the new equilibrium [] If K stays at 2?
To set up the ICE (Initial-Change-Equilibrium) chart, you need to keep in mind the stoichiometry of the balanced equation of the reaction and the given equilibrium concentrations.
Let's start by writing the balanced equation for the reaction:
N2O4(g) ⇌ 2NO2(g)
Given equilibrium concentrations:
[N2O4] = 2 M
[NO2] = 2 M
Since the stoichiometry of the reaction tells us that 1 mol of N2O4 produces 2 mol of NO2, we can infer that the change in concentration of N2O4 will be -2x (x being the change in concentration), and the change in concentration of NO2 will be +2x.
Now, let's consider the effect of decreasing the flask volume to 3 L. Since volume and pressure are inversely related (Boyle's Law), decreasing the volume will increase the pressure. This change in pressure will result in a shift in equilibrium to the side with the fewer moles of gas, according to Le Chatelier's Principle.
In this case, since the reaction produces two moles of NO2 for every mole of N2O4, there is a net decrease in moles of gas on the right-hand side of the reaction. Therefore, the reaction will shift to the right, producing more NO2.
To find the new concentrations at equilibrium, you can use the given equilibrium concentrations as the initial concentrations in your ICE chart. Since the volume has changed, you need to recalculate the new concentrations using the ideal gas law:
PV = nRT
In this case, you know the volume (3 L), the ideal gas constant (R), and the temperature (assumed constant), so you can solve for the new number of moles (n) in the system.
Once you have the new number of moles, you can divide by the new volume to find the new concentrations of N2O4 and NO2.
Finally, you can substitute these new concentrations into the equilibrium expression (K) and solve for x to determine the change in concentration and the new equilibrium concentrations of N2O4 and NO2.