SO2(g) + NO2(g) reverse reaction arrow 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.
---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?
How would you set this up? I tried to set it up using (4.1)(2.0+1.1)/(4.0-1.1)(.5+x) = 3, but got it wrong...and also tried (4.1-x)(2.0+x)/(4.0-x)(.5+X)=3...and also got it wrong...
Answered below. I can help find it if you can't.
So I found that you would have to set it up using (4.1)(3.1)/(2.9)(x-1.1). The x includes the .5 of NO2 already added, so to find how much was added to the original, find x and just subtract .5. The "x" value was the new initial value used to raise SO3 to 4.1 and that is why it is x-1.1.
To solve this problem, you need to apply the principles of equilibrium and use the given concentrations to determine the unknown concentration of NO2.
First, let's write the balanced chemical equation for the given reaction:
SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)
We are given the concentrations at equilibrium:
[SO2] = 4.00 M
[NO2] = 0.500 M
[SO3] = 3.00 M
[NO] = 2.00 M
Now, let's define the change in concentration of SO3 as x M:
[SO3] = 4.10 M = 3.00 M + x
In order to determine the change in concentration of NO2, we need to make an assumption regarding the change in concentration of NO. Since NO is in a 1:1 stoichiometric ratio with SO3, we can assume that its change in concentration will also be x M.
[NO] = 2.00 M + x
Now, using the ideal gas law, we can write an expression for the equilibrium constant, Kc:
Kc = ([SO3] * [NO]) / ([SO2] * [NO2])
Substituting the given concentrations, we have:
Kc = (3.00 M + x) * (2.00 M + x) / (4.00 M * 0.500 M)
To solve for x, we need to set up an equation:
Kc = (3.00 M + x) * (2.00 M + x) / (4.00 M * 0.500 M) = 3.00
Now you can solve this equation to find the value of x, representing the change in concentration of both SO3 and NO.
After obtaining the value of x, you can determine the moles/liter of NO2 that need to be added to the original equilibrium mixture by using the equation:
[NO2] = 0.500 M + x
Substitute the value of x into this equation to find the final concentration of NO2.
Remember to double-check your calculations and units to ensure accuracy.