# (1-16)Chemistry - Science

Consider the reaction:
SO2 (g) + NO2 (g) ==> SO3 (g) + NO (g)
At T = 1000 K, where the reaction is exothermic with an equilibrium constant K = 9.00

The reaction vessel is charged initially with all four gases, each at a pressure of 0.5 atm. After equilibrium is achieved, the partial pressure of SO3 will be:
a) 0.250 atm
b) 0.500 atm
c) 0.750 atm
d) 0.900 atm
e) none of these

1. First you must determine which way the reaction will shift to reach equilibrium.
Q = (SO3)(NO)/(NO2)(SO2) = (0.5*0.5/0.5*0.5) = 1. With K = 9 that means products are too small and reactants too large so the rxn must shift to the right to reach equilibrium.
.....SO2(g) + NO2(g) ==> SO3(g) + NO(g)
I...0.5.......0.5.........0.5.....0.5
C.....-x......-x..........x.......x
E...0.5-x...0.5-x........0.5+x...0.5+x

Substitute into Keq an solve for x, then evaluate each constituent.

posted by DrBob222

## Similar Questions

1. ### Chem Equilbirum

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
2. ### (1-17)Chemistry - Science

Consider the reaction: SO2 (g) + NO2 (g)  SO3 (g) + NO (g) At T = 1000 K, where the reaction is exothermic with an equilibrium constant K = 9.00 If the reaction vessel is instead charged initially with SO3(g) and NO(g),
3. ### Chemistry

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
4. ### Chem

Given the reaction: SO2(g) + NO2(g) = NO(g) + SO3(g) H = -42.6Kj How will the concentration of SO3 at equilibrium be effected by the following: a) Adding more NO2(g) b) Removing some NO(g) c) Increasing the temperature
5. ### Chemistry

The equilibrium constant is 16 for the gas phase reaction SO2 + NO2 <--> SO3 + NO at a certain temperature. If 3.0 moles each of SO2 and NO2 are placed together in an empty 1.0 liter flask and the system is allowed to come
6. ### Chemistry

At a given temperature, analysis of an equilibrium mixture represent below is given as: SO2(g) + NO2(g) <--> SO3(g) + NO(g) Where [SO2]=4.0M, [NO2]=0.50M, [SO3]= 3.0M, [NO]=2.0M. Find the value of Keq
7. ### Chemistry

Given the following equation: SO2 + NO2 <--> SO3 + NO At 25 Celcius, 2.00 mol of each of SO2 and NO2 are introduced into a 1.0L sealed flask. When euilibrium is reached, it is found that [NO2] = 1.30 mol/L [SO3] = 1.30 mol/L
8. ### chemistry

I am a bit confused with this proble because the concentration of SO3 at equilibrium. Any help would be appreciated. Given the reaction: SO2(g) + NO2(g) ⇌ NO(g) + SO3(g) ∆H = -42.6 kJ. How will the concentration of
9. ### Chemistry

An equilibrium mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 3.77 10-3 mol/L, [O2] = 4.30 10-3 mol/L, and [SO3] = 4.13 10-3 mol/L. Calculate the equilibrium constant, K, for the
10. ### Chemistry

At a particular temperature, K=3.75 for the following reaction. SO2(g) + NO2(g) (reversible arrows) SO3(g) + NO(g) If all four gases had initial concentrations of 0.500 M, calculate the equilibrium concentrations of the gases.

More Similar Questions