Consider the following system at equilibrium where h° = 198 kj, and kc = 2.90×10-2, at 1.15×103 k. 2so3(g) 2so2(g) + o2(g) if the volume of the equilibrium system is suddenly decreased at constant temperature: the value of kc c a. increases. b. decreases. c. remains the same. the value of qc b a. is greater than kc. b. is equal to kc. c. is less than kc. the reaction must: b a. run in the forward direction to reestablish equilibrium. b. run in the reverse direction to reestablish equilibrium. c. remain the same. it is already at equilibrium. the number of moles of o2 will: a a. increase. b. decrease. c. remain the same.

explanation: no but i do not usually comment

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.

the answer is a! (2.9 x 10^-18 j) hope i could someone. : )