For elementary reaction, order of reaction is sum of stoichiometric coefficient.
So rate law for given reaction,
Rate = K[H2O]
(d) is correct option.
Question 17 (1 point) C Determine the rate law for the following elementary reaction: H20H+OH. rate-k[H20]2...
Question 1 Select the rate law for the following reaction CH3CH2CH2CH2Br + OH → CH3CH2CH2CH2OH + Br- O a. Rate = k [RBr]? [OHT? b. Rate = k [RBr] [OH-12 c. Rate = k [RBr]> [OH) d. Rate = k [RBr] [OH] e Rate = k [RBr]
8. The rate law for the reaction H2O2 + 2H+212 + 2H2O is rate-k[H202][1]. The following mechanism has been suggested. H2O2+1 - HOI + OH - slow OH + H H20 fast HỘI + H+ + + I2 + H2O fast Identify all intermediates included in this mechanism. A) H and I D) Honly B) H and HOI E) H20 and OH C) HOI and OH 9. Which of the following statements is false? A) A catalyst increases the rate...
predict the product 1. (12 pts) Predict the product for the following transformation. OH OH 유 1.H2OH' HO 2. KH, 18-c-6, THF OH OH Br Ph OH OBn O 1. H20, H HO 2. O 、Me , cat. H+ Me 1. (12 pts) Predict the product for the following transformation. OH OH 유 1.H2OH' HO 2. KH, 18-c-6, THF OH OH Br Ph OH OBn O 1. H20, H HO 2. O 、Me , cat. H+ Me
What is the rate law for the elementary termolecular reaction 3A products? Rate -k[A] Rate -k[A] Rate = K[A]
The reaction below is an elementary reaction. What is the rate law of the reaction? Ca++ (aq) + Mn2+ (aq) → Ce+ (aq) + Mn3+ (aq) Rate = k[Cet] [Mn2+1 Rate = k[Ce**1? [Mn2+12 Rate = k[Ce 4+][Mn2-12 Rate = k[Ce**]? [Mn?")
Question 8 Step 1: H,02 + I +10- +H,0 Step 2: H,02 + 10 + H2O + O2 +I" The mechanism for a chemical reaction is shown above. Which of the following statements about the overall reaction and rate laws of the elementary reactions is correct? The chemical equation for the overall reaction is 2 H202 + I and the rate law for elementary step 2 is rate = k[H,02][10 + 2 H2O + O2 +I , ]. + H2O...
Write the rate law for the two elementary reaction equations. 2 A(g) + B(g) → C(g) +D(8) ratek X(g) + Y() - (8) rate =k
Question Determine the rate law and the value of k for the following reaction using the data provided. 1/1 point 2 N2O5 - 4 NO2+O IN20sl (M) initial Rate (M-1,-1) 0.093 4.84 x 10-4 0.084 4.37 x 10-4 0.224 1.16 x 10-3 Rate - 6,0 x 10-1M2-1N205) Rate -5.2 x 10-3541N205) Rate - 5.6 x 10 2 M15-41N20512 Rate - 1.6 x 10-3 M1/2,-41N20511/2 Rate - 1.7* 10-2M-1/2--IN20513/2
8) A reaction occurs via the following sequence of elementary steps. What is the rate law based on this reaction mechanism? very fast slow fast 1st step: A B 2nd step: B+C D 3rd step: D - 2E A) rate = k[E]2 B) rate = k[A] [C] C) rate = k[B][C] D) rate = k[D] E) rate = k[A] [B]
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...