Consider the following mechanism:
H2S <--> H+ + HS- (fast equilibrium)
Cl2 + HS --> 2Cl- + H+ + S (slow)
An intermediate is
And the best rate law is
Consider the following mechanism: H2S <--> H+ + HS- (fast equilibrium) Cl2 + HS --> 2Cl- + H+ + S (slow) An intermediate is And the best rate law is
consider the aqueous reaction of Cl2 + H2S -> S + 2HCL . It may happen by the following mechanism 1: Cl2-> <- 2Cl fast 2: Cl+H2S -> <- HCl + HS fast 3: HS +Cl --> --< HCl + S slow DERIVE a rate law for overall reaction using the given mechanism and rate determining step without using intermediates in the rate law.
The proposed mechanism for a reaction is Cl2 => Cl+ + Cl- Slow Cl- + H2S => HCl + HS- Fast Cl+ + HS- => HCl + S Fast Which of the following would be a rate law for the reaction? A. rate = k[Cl2] B. rate = k[Cl2][H2S] C. rate = k[Cl2]1/2[H2S] D. rate = k[Cl-][H2S] E. rate = [Cl+][Cl-]
Consider the following three step mechanism for a reaction Cl2 > 2Cl Fast Cl+CHCl3 > HCl+CCl3 Slow Cl+CCl3 > CCl4 Fast What is the predicted rate law? How do you do it? The answer is rate=K[Cl2]^.5 [CHCl3]
3.(12pts) The reaction Cl(aq) + HS(a) determined DRL S)+(aq) +2 Cl(aq) has the experimentally rate k[Cl2][H2S] Which of the following mechanisms is(are) consistent with the experimental results. Mech I Mech 11, Mech III Cl2 +H2S >H CI CI+HS (slow) CI+ + HS. …>H+ + Cl. + S H2S = HS. + H+ HSCl2 2CI +S+H (fast) (fast equil) (slow) H2S HS+H (fast equil) (fast equil) (slow) 4. (10 pts) Write the equilibrium constant Ke expression for the following 4 KO:(s)...
Consider the following mechanism: A2B (rapid equilibrium) B + 2C + E (slow) E F (fast) Which one of the following experimentally determined rate laws is consistent with this reaction mechanism? Multiple Choice Rate = KALC2 O Rate = KAVB2 O Rate = K[AIC] O Rate = MBIC2 Rate = ka]1/2012 O
Consider the reaction 2 NO + Cl2 → 2 NOCI A possible mechanism is: Cl2 ⇄ 2 Cl (fast) Cl + NO → NOCl (slow) If this is correct, the rate law will be: A. rate = k [NO]0.5[Cl] B. rate = k [NO]2[Cl2] C. rate = k [NO][Cl2] D. rate = k [NO][Cl]2 E. rate = k [NO][Cl2]0.5
Part A= Given the two reactions H2S⇌HS−+H+, K1 = 9.42×10−8, and HS−⇌S2−+H+, K2 = 1.32×10−19, what is the equilibrium constant K final for the following reaction? S2−+2H+⇌H2S Part B= Given the two reactions PbCl2⇌Pb2++2Cl−, K3 = 1.89×10−10, and AgCl⇌Ag++Cl−, K4 = 1.23×10−4, what is the equilibrium constant K final for the following reaction? PbCl2+2Ag+⇌2AgCl+Pb2+
Part A Given the following proposed mechanism, predict the rate law for the overall reaction. 2 NO2 + Cl2 → 2 NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast Given the following proposed mechanism, predict the rate law for the overall reaction. 2 NO2 + Cl2 → 2 NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast Answer Choices: Rate =...
Consider the following mechanism. step 1 2A > B slow B+ C D fast step 2 overall: 2A+C D Determine the rate law for the overall reaction (where the overall rate constant is represented as k) rate=
Consider the reaction 2 NO + Cl2 + 2 NOCI A possible mechanism is: Cl2 = 2 CI (fast) CI + NO NOCI (slow) If this is correct, the rate law will be: O A. rate = k [NO]?[C12] B. rate = k [NO][C12] C. rate = k [NO][CIT? D. rate = k [NO][C1270.5 E. rate = k [NO]0.5[CI] Reset Selection