For the reaction NO2(g) + NO(g) = N2O3(g)
If at particular temperature, K was 575 and equilibrium concentration of N2O3(g) was 2.5 M, calculate the equilibrium concentrations of NO2(g) and NO(g) if they both had the same initial concentrations.
i have my table layed out like...
NO2 + NO = N2O3
Inital concentration 2.0 2.0 0
Change concentration 2.5
Equilibrium concent. 2.5
I am stuck on how to finish the table.
Please help me!
NO2 + NO = N2O3
Inital concentration 2.0, 2.0, 0
Change concentration , ,2.5
Equilibrium concent. , ,2.5
Sarah, the problem doesn't say the initial concns of NO and NO2 were 2.0M. Did you just choose those numbers from the sky? I would do it this way.
.............NO2 + NO ==> N2O3
initial.......x.....x......0
change.......-2.5..-2.5...+2.5
equil.....x-2.5...x-2.5....2.5
575 = (N2O3)/(NO)(NO2)
675 = (2.5)/(x-2.5)(x-2.5) and solve for x. The EASY way to do that is to take the square root of both sides. I get approximately 0.066M
Thank you Doctor Bob this helped a lot i got the answer so i must have done something right :)
To calculate the equilibrium concentrations of NO2(g) and NO(g), you can use the concept of stoichiometry and the given equilibrium constant (K).
From the balanced equation:
NO2(g) + NO(g) = N2O3(g)
The stoichiometry tells us that for every 1 mole of N2O3 produced, 1 mole of NO2 and 1 mole of NO are consumed. Based on this, we can assume that the change in concentration for NO2 and NO is the same.
Given that the equilibrium concentration of N2O3(g) is 2.5 M, and the initial concentration of NO2(g) and NO(g) is both 2.0 M, we can use the values to fill in the table you provided:
NO2 + NO = N2O3
Initial concentration 2.0 2.0 0
Change concentration -2.5 -2.5 +2.5
Equilibrium concent. 2.0 -2.5 2.0 -2.5 2.5
Since the change in concentration of NO2 and NO is the same as the change in concentration of N2O3, we subtract 2.5 M from the initial concentration to get the equilibrium concentration.
Thus, the equilibrium concentrations of NO2(g) and NO(g) would both be 2.0 - 2.5 = -0.5 M.
Note that negative concentrations are not physically meaningful, so the equilibrium concentrations of NO2(g) and NO(g) should be considered as 0 M in this case.