- #1

BrettJimison

- 81

- 5

## Homework Statement

Rxn: 2SO

_{2}

_{(g)}+ O

_{2}

_{(g)}[itex]\Leftrightarrow[/itex] 2SO

_{3}

_{(g)}

If the initial concentration of SO

_{3}is .500 M (moles/liter) @1500K, what are the final concentrations of [SO

_{2}], [O

_{2}] and [SO

_{3}]. K

_{c}= .15

Stop when you get to the cubic equation

## Homework Equations

RICE table

K

_{c}= [SO3]

^{2}/ [O2][SO2]

^{2}This is equilibrium quotient for forward reaction. I will flip it to get reverse reaction Kc equation

## The Attempt at a Solution

This is the K

_{c}given for the forward reaction. If I flip the reaction around I invert the K

_{c}and it becomes = 6.6667 (for the reverse reaction)

I then used a "rice" table with the initial concentration of SO3 and "x" variable for the SO2 and O2[

Plugging these values in I get the kc equation:

6.6667= [2x]

^{2}[x]/[.500-2x]

I'm not getting the correct cubic equation when expanding this quotient. I'm sure of my math, so I was wondering if I'm setting up the quotient wrong? - Thanks!