|
Trial |
Initial [A] (M) |
Initial [B] (M) |
Initial Rate of disappearance of [A] (M/sec) |
|
1 |
0.015 |
0.200 |
3.67 × 10-6 |
|
2 |
0.030 |
0.200 |
1.47 × 10-5 |
|
3 |
0.015 |
0.400 |
7.34 × 10-6 |
above is the initial rate experimental data for reaction 2 A + 3 B -> 2 C + D
the special rate constant k of the reaction is:
Trial Initial [A] (M) Initial [B] (M) Initial Rate of disappearance of [A] (M/sec) 1 0.015...
For reaction 2A + 3B → 2C + D, following data of concentration and rate was obtained Trial Initial [A] Initial [B] Initial Rate (M/sec) 1 0.015 M 0.200 M 3.67 x 10^-6 20.030 M 0.200 M 7.33 x 10^-6 30.015 M 0.400 M 1.47 x 10^-5 The special rate constant k = A 1.2 x 10^-3 (1/M.sec) 9.2 x 10^-4 (1/M-sec) C 1.6 x 10^-3 (1/M-sec) 6.1 x 10^-3 (1/M^2-sec) E 8.2 x 10^-3 (1/M^2-sec)
1. Consider the reaction 2H2 + O2 + 2H2O What is the ratio of the initial rate of the appearance of water to the initial rate of disappearance of oxygen? a) 1:1 b) 2:1 c) 1:2 d) 2:2 e) 3:2 Garance of water to the initial rate of disappearance of oxyge 2. Consider the reaction X Y Z Which of the following is a possible rate law? a) Rate = k[X] Rate = k[Y] Rate = k[Y][Z] Rate = k[X][Y]...
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Consider the reaction of peroxydisulfate ion (S2O8^2-)(Aq) with iodide ion (I-) in aqueous solution: (S2O8^2-)(Aq)+(3I-)(Aq)---->2SO4^2-+(I3-)(Aq).At a particular temperature the rate of disappearance of S2O8^2 varies with reactant concentrations in the following manner:Experiment S2O8^2- I- Initial Rate1 0.018 0.036 2.6x10^-62 0.027 0.036 3.9x10^-63 0.036 0.054 7.8x10^-64 0.050 0.072 1.4x10^-51) Determine the rate law for the reaction.Apparently the rate law is Rate=[S2O8^2-][I-]How did they come up with this?2)How is the rate of disappearance ofS2O8^2- related to the rate of disappearance of [I-]...
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± Experimental Determination of a Rate Law Part B: Calculate the initial rate for the formation of C at 25 ∘C, if [A]=0.50M and [B]=0.075M. Express your answer to two significant figures and include the appropriate units. Consider the reaction A+2B⇌C whose rate at 25 ∘C was measured using three different sets of initial concentrations as listed in the following table: Trial [A] (M) [B] (M) Rate (M/s) 1 0.50 0.030 9.0×10−3 2 0.50 0.060 1.8×10−2 3 1.00 0.030 3.6×10−2
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Using the given data, calculate the rate constant of this reaction. A+B⟶C+D Trial [A] (M) [B] (M) Rate (M/s) 1 0.300 0.400 0.0227 2 0.300 1.08 0.165 3 0.450 0.400 0.0341 STRATEGY: Determine the rate law. Solve the rate law for ?, and calculate the ? value. Step 1: What is the rate law in terms of ? , [A] , and [B] ? Rate=__________