Chemistry
posted by Andre on .
SO2(g) + NO2(g) SO3(g) + NO (g)
At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M.
(a) What is the new equilibrium concentration of NO when 1.50 moles of NO2 are added to the equilibrium mixture? Assume a 1.00 L container.
[NO] = 2.84M <<answer
(b) How many moles/liter of NO2 would have to be added to the original equilibrium mixture to increase the equilibrium concentration of SO3 from 3.00 M to 4.10 M at the same temperature?
[NO2] =?????????????/
i need help on part b how do u do this? thanks!!

K = [SO3][NO]/[SO2][NO2]
K = (3.0)(2.0)/(4.0)(0.5)= 3.0
(a) Some of the added NO2 will be used up causing a shift to the right. Let that be equal to x.
At the new equilibrium,
[SO2]=4.0x, [NO2]=0.5+1.5x=4.0x
[NO]=2.0+x, [SO3]=3.0+x,
Set up:
K = [3.0+x][2.0+x]/[4.0x][2.0x]
Simplify and solve for x
[NO]=2.0+x
(b)
Let the moles of NO2 added = x
Set up:
3.0 = [3.0+1.1][2.0+1.1]/[4.01.1][0.5+x]
Solve for x 
I tried to answer the hwk using this tip for part B, but I didn't get it right...is there another way to set it up?

SO2(g) + NO2(g) SO3(g) + NO (g)
At a given temperature, analysis of an equilibrium mixture found [SO2] = 0.300M, [NO2] = 0.100 M, [SO3] = 0.600 M, and [NO] = 2.00 M. At the same temp., extra SO2 was added to make SO2 is added to make [SO2}= 0.800M. Calculate the composition of the mixture when equilibrium has been reestablished