A compare? rate Coastant at 1.000 x 10k, and 2. The reaction CO(g) + Cl2 →...
5. Consider this 2-step mechanism for a reaction. NO2(g) + Cl2(g) k1 ClNO2 (g) + Cl(g) Slow NO2(g) + Cl(g) k2 ClNO2(g) Fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. What is the predicted rate law?
The formation of phosgene CO + Cl2 → COCl2 is thought to proceed by the following mechanism ( 1) Cl2 → 2 Cl K1 (equilibrium constant for step 1) (2) Cl + CO → COCl K2 (equilibrium constant for step 2) (3) COCl + Cl2 → COCl2 + Cl k (rate constant for step 3) Find the rate law R = dt [COCl2 ] / dt = ?
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.
please note step 2, the right side if the equation is supposed
to read:
CO + Cl + M Step 2
CO(g) + Cl2(g) = COCl2(g) Given the mechanism below, answer the following questions. Cl2 + M 2CI+ M Cl + COM COCI + M COCI + Cl2 COCl2 + c Step 1 Step 2 Step 3 a. There are two intermediates in this mechanism. Identify them. b. In terms of the product molecule write an expression for the rate...
1. The rate of formation of carbon tetrachloride from chloroform, CHCl3(g) + Cl2(g) => CCl4(g) + HCl(g) is first order in CHCl3 and half order in Cl2. Which step of the proposed mechanism must be slow in order to agree with this rate law? 1. Cl2(g) => 2 Cl(g) 2. Cl(g) + CHCl3(g) => HCl(g) + CCl3(g) 3. CCl3(g) + Cl(g) => CCl4(g) 1. 1 2. 2 3. 3 2. The proposed mechanism for a reaction is Cl2 =>...
Consider the following two-step mechanism for a reaction: NO2(g)+Cl2(g)→ClNO2(g)+Cl(g)Slow N O 2 ( g ) + C l 2 ( g ) → C l N O 2 ( g ) + C l ( g ) S l o w NO2(g)+Cl(g)→ClNO2(g)Fast a)What is the overall reaction? Express your answer as a chemical equation. Identify all of the phases in your answer. b)Identify the intermediates in the mechanism. Check all that apply. Check all that apply. NO2(g), ClNO2(g), Cl2(g) ,Cl(g)...
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 =...
1) For the reaction; CO (g) + Cl2 (g)→ COCl2 (g) K= 215 If I start with 2.50 M CO and 3.50 M chlorine calculate the equilibrium concentrations of all three chemicals. 2) How long will it take for 23% of a chemical to decompose if the process is first order and I am starting with 3.0M with a half life of 2.1 years? Please answer in years. 3) Write the overall rate law for the following series of reactions;...
Consider the following reaction: COCl2(g) = CO(g) + Cl2(8) A reaction mixture initially contains 1.6 M COC12. Determine the equilibrium concentrations of COCI, CO, and Cl2 if Kc for the reaction at this temperature is 8.33 x 10-4. Calculate this based on the assumption that the answer is negligible compared to 1.6. Use x is small approximation. Show Q Validity check [Cl2] = [CO]= [COCI2] = Calculate the reaction quotient, Q A % Validity Check A Calculate the A/ equilibrium...
The following mechanism has been proposed for the gas-phase reaction of chloroform (CHCl3) and chlorine. Cl2 ⇌ 2Cl (fast, reversible) Cl + CHCl3 → HCl + CCl3 (slow) Cl + CCl3 → CCl4 (fast) What rate law does this mechanism predict? (Choose from the list below and enter your answers in alphabetical order, e.g. ABC ). A)k G) [CHCl3]1/2 M) [CCl3]2 B) [Cl2] H) [CCl3]1/2 N) [HCl]2 C) [Cl] I) [HCl]1/2 O) [Cl2]2 D) [CHCl3] J) [Cl2]1/2 P) [Cl]2 E)...