Thursday
July 31, 2014

Homework Help: Chemistry

Posted by Jeena on Monday, March 29, 2010 at 5:16pm.

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...

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

Chem Equilbirum - SO2(g) + NO2(g) reverse reaction arrow SO3(g) + NO (g) At a ...
Chemistry - SO2(g) + NO2(g) SO3(g) + NO (g) At a given temperature, analysis of ...
Chemistry - At a given temperature, analysis of an equilibrium mixture represent...
Chemistry - The equilibrium constant is 16 for the gas phase reaction SO2 + NO2...
chemistry - I am a bit confused with this proble because the concentration of ...
Chemistry - Given the following equation: SO2 + NO2 <--> SO3 + NO At 25 ...
Chemistry - At a particular temperature, K=3.75 for the following reaction. SO2(...
Chem - Given the reaction: SO2(g) + NO2(g) = NO(g) + SO3(g) H = -42.6Kj How will...
Chemistry - At a certain temperature, the equilibrium constant for the following...
General Chemistry - At a certain temperature, the equilibrium constant for the ...

Search
Members