To find K, simply measure the concentrations of products and reactants and use equilibrium expression
For O2 + 2SO2 ⇄ 2SO3 where the equilibrium concentration are [O2] = 2x10^-8 M, [SO2] = 3.4x10^-9 M, and [SO3] = .971 M
Reaction | NO2 | + | SO2 | ⇄ | NO | + | SO3 |
---|---|---|---|---|---|---|---|
Inital [ ] | |||||||
Change | |||||||
Eqlbrm | |||||||
Answer |
Reaction | NO2 | + | SO2 | ⇄ | NO | + | SO3 |
---|---|---|---|---|---|---|---|
Inital [ ] | .250M | .250M | .250M | .250M | |||
Change | -x | -x | +x | +x | |||
Eqlbrm | .250 -x | .250 -x | .250+x | .250 +x | |||
Answer |
Reaction | NO2 | + | SO2 | ⇄ | NO | + | SO3 |
---|---|---|---|---|---|---|---|
Inital [ ] | .250M | .250M | .250M | .250M | |||
Change | -x | -x | +x | +x | |||
Eqlbrm | .250 -x | .250 -x | .250+x | .250 +x | |||
Answer | .261M | .261M | .239M | .239M |
Plugging the answer values to the equilibrium expression:
At equilibrium, the chemical reaction obeys the equilibrium expression and the expression can be used to calculate the concentrations
For the reaction H2 + I2 ⇄ 2 HI, where K = 49, [I2] = .2M, [HI] = .05M, [H2] can be calculated:
Rxn | Br2 | + | Cl2 | ⇄ | 2BrCl |
---|---|---|---|---|---|
Initial [ ] | 0M | 0M | .2M | ||
Change | -x | -x | +2x | ||
Eqlbrm | -x | -x | .2M - 2x | ||
Answer |
For the reaction H2 + I2 ⇄ 2HI, the Kp expression is
For the reaction 2S + 3O2 ⇄ 2SO3 where the partial pressure are S = .0035atm, O2 = .0021atm, and SO3 = .005atm, what’s the Kp?
Kp = Kc(RT)^(Δng)
For the reaction 2NO (g) + O2 (g) ⇄ 2 NO2 (g) where the Kc is 5.6x10^12 at 290K, what’s the Kp?
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