For the chemical reaction
Mn2+ (aq) + H2O2 (aq) ---> products
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[Mn2+], M [H2O2], M Initial rate [M/s]
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0.740 0.556 3.43x10-2
0.219 0.556 3.01x10-3
0.740 0.662 4.86x10-2
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Determine the order with respect to Mn2+ and H2O2, and construct the complete rate law, including the value of the rate law constant.
For the chemical reaction Mn2+ (aq) + H2O2 (aq) ---> products _______________________________________________________________ [Mn2+], M [H2O2], M &nbs
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From the stoichiometry of the reaction 2 I– (aq) + H2O2 (aq) + 2 H3O+ (aq) I2 (s) + 4 H2O (l) What can be said about rate law for this reaction? Explain the answer. a. The rate law is predicted to have a molecularity of five. b. The rate law is predicted to be second order in [I–]. c. The rate law is predicted to be first-order in [H2O2]. d. Statements a, b, and c are all true....
3. For the reaction, H2O2 (aq) + 3 (aq) + 2 H (aq) → 2 H20 (1) + 1- (aq) Ot The rate law was experimentally determined to be Rate = k[H2O2][T] a. What is the reaction order in terms of H20,? b. What is the reaction order in terms of I? because et is nuoto c. What is the reaction order in terms of HT? O d. What is the overall reaction order of this reaction? 4. If a...
2 HgCl2(aq) + C2O42-(aq) → 2 Cl-(aq) + 2 CO2(g) + Hg2Cl2(s) Experiment [HgCl2], M [C2O42-], M Initial rate 1 0.105 0.15 1.8 x 10-5 2 0.105 0.30 7.1 x 10-5 3 0.052 0.30 3.5 x 10-5 4 0.052 0.15 8.9 x 10-6 a) Determine the order of reaction with respect to HgCl2. b) Determine the order of reaction with respect to C2O42-. c) Determine the overall order of the reaction. d) What is the rate law? e) Determine the...
The following reaction was studied experimentally at 25 °C. S2O82(aq) + 21'(ag) = 12(aq) + 2SO4 (aq) The reaction was found to be first order with respect to I and first order with respect to S208". A reaction was performed with [1] = 0.080 M and [S208²-] = 0.040 M. The initial rate of formation of 12 was found to be 1.25 x 10-M St. Provide an expression for the rate law for this reaction and determine the initial rate...
Consider the balanced chemical equation. H2O2(aq)+3I−(aq)+2H+(aq)→I3−(aq)+2H2O(l) In the first 14.0 s of the reaction, the concentration of I− drops from 1.000 M to 0.817 M Predict the rate of change in the concentration of H2O2 (Δ[H2O2]/Δt). Express the rate to three significant figures and include the appropriate units. (I understand the arithmetic, but I'm having a tough time with the units)
5. Given the reaction OCT (aq) + I (aq) → OT (aq) + Cl(aq) tienis Rate = k1110017. Th The rate law for this reaction is Rate =k! . The overall reaction order and the [OH"] order with respect to OH are A) 2 and -1. B) O and -1. C) 0 and 1. D) 2 and 1. E) 1 and -1. 6. The following data were obtained for the hypothetical reaction 2A + B → products, [A] (M) [B]...
1. Why is the starch indicator added to the reaction solution? 2. Consider the following balanced chemical reaction: 2 MnO, (aq) + 5 H2O2(aq) + 6 H*(aq) → 2 Mn2+ (aq) + 5 O2(g) + 8 H,O(1) a. A student wrote the following rate law for this reaction: Rate = k [MnOz]”[H202]*[H+]6 Is this correct? Explain. b. Briefly describe what must be done to obtain the correct rate law. 3. Define the following terms: a. Rate: b. Rate law: c....
GIVEN THE FOLLOWING DATA FOR THIS REACTION: NH4+(aq) + NO2-(aq) ---> N2(g) + 2H2O(l) EXPT NH4+ NO2- RATE 1 0.010 M 0.020 M 0.020 M/s 2 0.015 M 0.020 M 0.030 M/s 3 0.010 M 0.010 M 0.005 M/s a. Calculate the order of reaction with respect to NH4+ b. Calculate the order of reaction with respect to NO2- c. Calculate the rate constant k d. Determine the overall order of reaction e. Determine the rate law