Consider the reaction: H2O(g) + CO(g) H2(g) + CO2(g) Which of the following statements are true and which are false. false Reactions with large equilibrium constants are always slow. false When Q > K the system will spontaneously shift to the right. false Amounts of all reactants and products corresponding to an exact equilibrium composition for this reaction are sealed in a vessel. The CO placed in the vessel is labelled with 14C. After an indefinite period of time 14C would still be found only in the CO molecules and not in CO2. false 1 mol of H2O(g) and 1 mol of CO(g) are placed in a vessel and 1 mol of H2(g) and 1 mol of CO2(g) are placed in another of equal volume. At equilibrium, at 350°C, the amounts of CO(g) in the two vessels are equilvalent. true At equilibrium, the overall composition of the reaction mixture is not changing. false At equilibrium, individual molecules cannot undergo any chemical reactions. HI can someone chek those for me, there is/are some wrong answer there but i cannot seem to figure it out. If someone can see it please help!!