Experiment | [A]o (M) | [B]o (M) | [C]o (M) | Rate -dA/dt (M/s) |
1 | 0.5 | 1.0 | 1.0 | 6.4 |
2 | 1.0 | 1.0 | 1.0 | 12.8 |
3 | 0.5 | 0.5 | 1.0 | 6.4 |
4 | 0.5 | 1.0 | 2.0 |
25.6 |
What is the order of reagent A?
What is the order of reagent B?
What is the order of reagent C?
What is the rate law of the reaction?
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Experiment [A]o (M) [B]o (M) [C]o (M) Rate -dA/dt (M/s) 1 0.5 1.0 1.0 6.4 2...
Products yielded the following data: 6. A reaction A+B+C Initial concentration (mmol L-1) Initial rate (-d[Al/dt) (mmol L-1 s-1) Experiment AI) 0 [C]O Initial rate (-dA/dt mM I-S-1) [BJO 8.72 11.25 1.25 1.25 2.50 1.25 1.25 17.4 3 1.25 3.02 1,25 50.84 3.75 457 1.25 3.02 a) Write the rate law for this reaction b) If the initial reactant concentrations were [A]0 2 mmol L-1, [Bl0 1.5 mmol L-1 and [C]0 =1.15 mmol L-1, indicate what would be the initial...
Given the following initial rate data, write the rate law expression. Experiment [A]o, M [B]o, M Initial rate, M/s 1 5.1 × 10-4 0.35 × 10-4 3.4 × 10-8 2 5.1 × 10-4 0.70 × 10-4 6.8 × 10-8 3 5.1 × 10-4 0.18 × 10-4 1.7 × 10-8 4 1.0 × 10-3 0.35 × 10-4 6.8 × 10-8 5 1.5 × 10-3 0.35 × 10-4 10.2 × 10-8 A. k [A] [B] B. k [A]2 [B]2 C. k [A]2...
The following data were obtained for the reaction A+B → products: Experiment [A]O [B]O Initial rate, v (mol L''s') 2 3 1.25 x 10-3 M 1.25 x 10-3 M 12.50 x 10-3 M 1.25 x 10-3 M 1.25 x 10-3 M 3.13 x 10-3 M 3.01 x 10-3 M1.00 x 10-3 M 0.0087 0.0174 0.0544 4 ? 10.) Write the rate law for the reaction. Explain your reasoning in arriving at your rate law. (Hint: Table 1 is useful here.]...
2 ICl + H2----->I2 + 2 HCl Experiment [ICl]o, M [H2]o, M Initial Rate, M s-1 1 0.129 8.70×10-2 1.67×10-3 2 0.258 8.70×10-2 3.34×10-3 3 0.129 0.174 6.68×10-3 4 0.258 0.174 1.34×10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = ____________ From these data,...
Experiment Initial [A] Initial [B] Initial [C] Initial Rate of Reaction 1 0.1 M 0.1 M 0.2 M 4 x 10^(-4) M/min 2 0.3 M 0.2 M 0.2 M 1.2 x 10^(-3) M/min 3 0.1 M 0.3 M 0.2 M 4 x 10^(-4) M/min 4 0.3 M 0.4 M 0.6 M 3.6 x 10^(-3) The method of initial rates is used to determine the rate law for reactants A, B, and C. This data was obtained at 25 degrees C....
A + 2B-30 Experiment Number [A] (M) [B] (M) Initial Rate (M/s) 1 0.112 0.58 0.87 2 0.112 1.16 1.74 3 0.560 0.58 21.75 The rate law for this reaction is rate ОА. k[A]2[B] O B. [P] Ock[A][B] OD [A]2 O E k[A]2[B]2
The experimental data below were obtained. Experiment # [A] (M) [B] (M) Initial Rate (M/s) 1 1.80 3.54 4.52 2 1.80 7.08 4.52 3 5.40 3.54 40.68 What is the rate law for this reaction?
The reaction A B + 2 C is known to be zero order in A and to have a rate constant of 3.0 x 10–1mol/L. An experiment was run at 25°C and initial concentration of reagent [A] = 2.0 x 10–3 M. What is the rate of the reaction? Unable to predict. The rate of the reaction is 3.0 x 10–1 mol/L. The rate of the reaction is 2.0 x 10–3 mol/L. The rate of the reaction is 6.0 x 10–4 mol/L.
2NO(g) + Br2(g) = 2NOBr(g) Experiment [NO-] (M) [Br2] (M) Initial Rate (M s-1) 1 0.10 0.20 24 2 0.25 0.20 150 3 0.10 0.50 60 4 0.35 0.50 735 1.) Determine the rate law equation for the reaction. 2.) What is the overall order of the reaction? 3.) What are the value and the units of the rate constant, k? 4.) Write the expression to show how is the rate of disappearance of bromine, Br2, related to the rate...
Data for the following reaction are given in the table. 2NO(g) + Br2(g)->2NOBr(g) Experiment [NO],M [Br2],M Initial rate, M/s 1 1.0x10-2 2.0 x10-2 2.4x10-2 2 4.0x10-2 2.0x10-2 0.384 3 1.0x10-2 5.0x10-2 6.0x10-2 What is the rate law for this reaction? b. What is the overall order of the reaction? c. What is the rate constant for this reaction?