# chemistry

posted by .

How will the following system at equilibrium shift in each of the following cases?

2 SO3(g) <--> 2 SO2(g) + O2(g) HÂ° = 197 kJ

(a) SO2(g) is added
(b) the pressure is decreased by increasing the volume of the container
(c) the pressure is increased by adding Ne(g)
(d) the temperature is decreased
(e) O2(g) is removed

• chemistry -

Don't you have some ideas about what happens. Remember, Le Chatelier's Principle says that when a system at equilibrium is subjected to a stress, the reaction will shift in such a way so as to relieve the stress.
I'll do the first one.
when SO2 is added (a product) what must the reaction do? It must shift so as to use up the SO2 that was added. How can it do that? It can shift to the left, using up some of the O2 and some of the SO2 and forming more SO3. That way the SO2 concentration (the material which stressed the equilibrium) is reduced. Now you try the others and give reasons.

## Similar Questions

1. ### Chemistry

EQUILIBRIUM: Given the equation 2 PbS(s) + 3 O2(g) 2 PbO(s) + 2 SO2(g) What direction will the reaction proceed if additional SO2 was added to the system at equilibrium?
2. ### P. Chemistry

The equilibrium 2 SO2(g) + O2(g) 2 SO3(g) has the value K = 2.5 1010 at 500. K. Find the value of K for each of the following reactions at the same temperature. (a) SO2(g) + 1/2 O2(g) SO3(g) K = (b) SO3(g) SO2(g) + 1/2 O2(g) K = (c) …
3. ### 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 following …
4. ### chemistry

An equilibrium mixture of SO2,SO3 and O2 gases is maintained in a 11.5 L flask at a temp at which Kc=55.2 for the rxn: 2SO2 + O2 <> 2SO3. If the # of moles of SO2 and SO3 are =, how many moles of O2 are present?
5. ### Chemistry(Urgent, please respond, thanks!!)

1) For the reaction system, 2 SO2(g) + O2(g) = 2 SO3(g), Kc has a value of 4.62 at 450.0 K (Kelvin). A system, at equilibrium has the following concentrations: (SO3) = 0.254 M; (O2) = 0.00855 M. What is the equilibrium concentration …
6. ### 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 following …
7. ### chem: equilibrium

In which direction does the equilibrium shift for the following reaction?
8. ### Chem

At 930 K, Kp = 0.30 for the following reaction. 2 SO2(g) + O2(g)=>2 SO3(g) Calculate the equilibrium partial pressures of SO2, O2, and SO3 produced from an initial mixture in which the partial pressures of SO2 and O2 = 0.51 atm …
9. ### Chemistry

What will happen to the number of moles of SO3 in equilibrium with SO2 and O2 in the following reaction in each of the following cases?
10. ### Chemistry

For the teaction system, 2SO2(g) + O2(g) <--> 2SO3(g), Kc has a value of 4.62 at 450.0K. A system, at equilibrium, has the following concentrations: [SO3] = 0.254 M, [O2] = .00855 M. What is the equilibrium concentration of SO2(g)?

More Similar Questions