- Which one of the following statements is not correct? (a) The value of equilibrium constant is changed in the presence of a catalyst in the reaction at equilibrium. (b) Enzymes catalyse mainly bio-chemical reactions. (c) Coenzymes increase the catalytic activity of enzyme. (d) Catalyst does not initiate any reaction.

Select all of the correct statements about equilibrium from the choices below.At equilibrium the rates of forward and reverse reactions are equal. As a reaction proceeds forward toward equilibrium the forward rate drops. At equilibrium all reactions stop.   Reactants are transformed into products even at equilibrium.   As a reaction proceeds forward toward equilibrium the reverse rate constant rises.As a reaction proceeds forward toward equilibrium the forward rate constant drops.

Write the equilibrium constant expression. Solid carbon and carbon dioxide gas react and form carbon monoxide: C(s) + CO₂(g) = 2CO(g)

Consider the following reversible reaction at equilibrium: C6H12O6(aq) + 6 O2(g)      6 CO2(g) + 6 H2O(l). Given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?

The following reactions all have K > 1. 1) CH3COO (aq) + C,H;COOH (aq) =CH;C0OH (aq) + CgH;C00 (aq) 2) CN (aq) + CgH;COOH (aq)= C,H3C00 (aq) + HCN (aq) 3) CH;COОH (аq) + CN (aq) — НCN (aq) + CH;COО (аq) Arrange the substances based on their relative base strength. Clear All C,H;COOH C,H;C00- strongest base CN- intermediate base CH3CO0 weakest base HCN not a Bronsted-Lowry base CH;COOH

Consider the following equilibrium for which H = 180.74: N2(g) + O2(g)  2 NO(g) How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction?(a) NO(g) is added to the system.       (b) The reaction mixture is cooled.       (c) The volume of the reaction vessel is reduced by 50%.       (d) A catalyst is added to the reaction mixture.       (e) The total pressure of the system is increased by adding a noble gas.       (f) O2(g) is removed from the system.

Acetaldehyde (CH3CHO) is an important chemical both industrially and biologically.  For instance, it is a (somewhat toxic) intermediate in the body's metabolism of ethanol into acetic acid, and thus is possibly implicated in the "hungover" symptoms of someone who has had too much to drink the night before.  In aqueous solution, it establishes an equilibrium with a hydrated form, shown below. CH3CHO (aq)   +   H2O (l)   <-->  CH3CH(OH)2 (aq) You start with an aqueous sample, already at equilibrium, with the CH3CH(OH)2 (the hydrated form) at a concentration of 2.60 M.  You have no information about how much, if any, of the anhydrous form (CH3CHO) is initially in the flask.  If you add 2.0 M of CH3CHO to the reaction flask, and as the equilibrium is being restored the amount of CH3CH(OH)2 changes by 1.13 M, what is the final amount of CH3CHO?

Compare the following two reactions ("A" and "B"), with two different equilibrium constants, K: (A) Cl2 (g) + H2 (g) = 2HCI (g) K = 0.29 (B) I2 (g) + H2 (g) = 2HI (g) K = 1.6 x 1033 %3D Which of the following statements is correct? O Reaction "A" will proceed faster because the equilibrium constant, K, is larger O Reaction "B" will proceed faster because the equilibrium constant, K, is larger O Reaction "A" favors the production of products. O Reaction "B" favors the production of products. O None of these statements are correct.