2SO2 + O2 ==> 2SO3
SO2 = 8.00 mols and (SO2) = 8.00/2 = 4.00M
O2 = 10.00 mols and (O2) = 10.00/2 = 5.00 M
(SO3) = 2x
(O2) = 5.00-x
(SO2) = 4.00-2x
Plug into the equilibrium constant expression and solve for x. Then you can calculate the other concentrations.
For part b, I'm sure you know this is based on the principle of Le Chatelier. Let me know what you don't understand about this and I can help you through it BUT I don't want to just give you the answers. For biii it may help if you write the equation as
2SO2 + O2 ==> 2SO3 + heat (since the problem states that the enthalpy is negative for the production of SO3). So if enthalpy is negative, that means delta H is minus and that means heat is given off so heat goes on the product side.
since there are 10.00 moles of sulfur trioxide, shouldn't the initial concentration of SO3 = 5.00 M? (you have it posted as O2 = 5.00 M)
And for part b, I'm having problems on letter iii. I don't understand how the equilibrium constant would be affected by temperature. Would the constant increase because the molecules move faster in a raised temperature, causing more production of SO3?
I see I can't read. It was late last night but I didn't know it was that late. Please excuse me and thank you for pointing out the obvious error.
On part biii. T almost ALWAYS affects K. In fact, the K of a reaction is evaluated at a particular T and it isn't good for other temperatures. As I pointed out last night, the reaction is exothermic since the problem states that the enthalpy is negative with respect to the production of SO3. Therefore, we may write the equaion as
2SO2 + O2 ==> 2SO3 + heat.
Now treat heat the same way you would a change in concentration of one of the reagents; i.e.,an increase in heat makes the reaction shift in such as way as to use up the added heat. That means it will shift to the left. Shifting to the left means (SO2) and (O2) will become larger and (SO3) will become smaller. Check me out on that. What does that do to K?
so since K= products/reactants, K will get smaller?
I definitely understand this concept better now. Thank you so much for your help!
You're welcome. Come back anytime.
which one of the following reactions is not balanced (1)2SO2+O2-2so2,(2)2co+02-2co2,(3)2kno3+10-5k2o+n2,(4)SF4+3H2O-H2so3+4HF
Answer this Question
Chemistry - Consider the following equilibrium at 1000K: 2SO2 (g) + O2 (g) ¡ê ...
Chemistry - according to the balanced chemical equation 2SO2<--- 2 is a ...
AP Chemistry - Sulfuric acid (H2SO4)is prepared commercially from elemental ...
Ap Chemistry - Sulfuric acid is prepared commercially from elemental sulfur ...
chemistry - Sulfur trioxide, SO3, is produced in enormous quantities each year ...
CHEMISTRY - 2H2S + 3O2 → 2H2O +2SO2 given the balanced equation, if 4 ...
chemistry - sulfur trioxide gas dissociates into sulfer dioxide gas and oxygen ...
CHEMISTRY HELP! - I am COMPLETELY LOST for this one...dnt even know where to ...
Chemistry - Sulfur trioxide gas, one of the causes of acid rain, is produced in ...
AP Chemistry - At a certain temperature, the equilibrium constant Kc is 0.154 ...