Given :
Order of reaction wrt A = 2
Order of reaction wrt B = 0
Overall order = 3
Order of reaction wrt C = ?
The overall order of a reaction is equal to sum of the individual orders of reaction of all the reactant taking part in chemical reaction
Overall order of reaction = order of reaction wrt A + order of reaction wrt B + order of reaction wrt C
3 = 2 + 0 + Order of reaction wrt C
Order of reaction wrt C = 3 – 2 = 1
Hence order of reaction wrt C is = 1
If the reaction 3A +B+C 2D + E is second order in A, zero order in...
Consider the following elementary steps that make up the mechanism of a certain reaction: 3A→B+C B+2D→C+F If the overall reaction is 3A+2D→2C+F, Which species is a reaction intermediate?
The reaction A + B → C + D is second order in A and zero order in B. The value of k is 0.012 M-1min-1. What is the rate of this reaction when [A] is 0.125 M and [B] = 0.435 M? A. 5 x 10-4 B. 3.4 x 10-3 C. 1.9 x 10-4 D. 1.3
For the reaction 3A + 6G - 2D + 3E, the following initial rates of reaction were found. [A]./M [G]/M Initial Rate of Reaction / (M/s) 0.517 0.107 8.40x10-1 0.172 0.107 9.33x10-2 0.517 0.0535 4.20x10-1 Determine the rate law, filling in the appropriate spaces below. R = K[A] Submit Answer [G] Tries 0/5 Determine the overall order of the reaction. Submit Answer Tries 0/5 This discussion is closed. Send Feedbach
6. Consider the reaction 3A - C. If the reaction is second order with a half-life of 20.00 hrs. Starting the reaction with an initial concentration of A as 0.75M, calculate the time required for the concentration to decrease to 0.25M (8 points)
A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. Part A Write a rate law for the reaction. O Rate = k [A] [B] [C]1/2 O Rate = k [B] [C]1/2 Rate = k [B]1/2 [C] Rate = k [A] [B]1/2 [C] Submit Request Answer Part B What is the overall order of the reaction? Express your answer numerically. EVO AEQ O 2...
6. Consider the reaction 3A C. If the reaction is second order with a half-life of 20.0) hrs. Starting the reaction with an initial concentration of A as 0.75M, calculate the time required for the concentration to decrease to 0.25M (8 points)
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If the b. first c. second 10. What is the order with respect to NO? 11. What is the order with respect to Ch? azero a. zero b b. first c. second d. third d. third is 1.37 103
14 of 15 The rate law for the reaction, A+B-C, that is zero order for both reactants is O rate=k O rate=k[A] O rate=k[A][B] O rate=k[C] 15 of 15 For a reaction that is second order in A, calculate the value of the rate law constant using the table below: Experiment Initial [A]/M Initial rate/M s 0.010 0.020 .040 0 win 0.012 .050 0.19 3 0 118 M-18-1 O 126 M-15-1 O 0.40 M-15-1 O 121 M-15-1
The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y=mx+by=mx+b. Order Integrated Rate Law Graph Slope 0 [A]=−kt+[A]0[A]=−kt+[A]0 [A] vs. t[A] vs. t −k 1 ln[A]=−kt+ln[A]0ln[A]=−kt+ln[A]0 ln[A] vs. tln[A] vs. t −k 2 1[A]= kt+1[A]01[A]= kt+1[A]0 1[A] vs. t1[A] vs. t k Part A The reactant concentration in a zero-order reaction was 8.00×10−2 MM after 130 ss and 4.00×10−2 MM after 380 ss . What is...