C2O4 (aq) + H2O2 (aq) + 2 H+ (aq) → 2 CO2 (g) + 2 H₂O (1)Use the experimental data in the table to determine the rate law for this reaction (allconcentrations in mol/L).Exp.[CO2][H₂O₂][H+]Rate (in M/s)123+0.3900.2250.1003.34x1060.7800.2250.1006.69x1060.3900.6750.1003.01x10-540.7800.2250.2001.33x10-5

Rate law,Rate=k[C2O4-2][H2O2]2[H+]Explanation:Where k=rate constant

Answered: C2O4 (aq) + H2O2 (aq) + 2 H+ (aq) → 2…

Chemistry

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The reaction, NO₂Cl(g) + CI(g) -> NO2(g) + Cl₂(g), was found to be first order in each of the two reactants and second order overall. The rate law is therefore rate = k[NO₂]² rate = k[NO₂][ Cl₂] rate = k[CI] rate = K[NO₂CI][CI][NO₂][C1₂] rate = K[NO₂CI][CI]
Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2C1O₂(aq) + 2OH (aq)- ClO₂ (aq) + CIO, (aq) + H₂O(1) Under a certain set of conditions, the initial rate of disappearance of chlorine dioxide was determined to be 2.30 x 10 M/s. What is the initial rate of appearance of chlorite ion under those same conditions? 5.75 x 10-² M/s 4.60 x 10-¹ M/s A B 1.15 x 10-¹ M/s 2.30 x 10-¹ M/s E 9.20 x 10-¹ M/s
Ff.34.
Express the rate of the reaction 2NO(g)+ O2(g)–→ 2NO2(g) a. in terms of ANO2]. rate = Η ΔΝΟ,1/Δt b. in terms of A[O2]. _ A[02]/At rate =
Given the following results: Rate of Run Reaction [1] (M/s) 1.76 0.358 0.476 4.72 0.358 0.843 5.25 0.672 0.476 1 2 3 [H₂O2] Calculate the rate constant(k) for each run. Assuming the Rate Law = k[1]²[H₂O₂] calculate the average rate constant,k, for this reaction. Give your answer to 2 places after the decimal.
Given the following results: Run Rate of Reaction (M/s) [I-] [H2O2] 1 1.99 0.516 0.561 2 3.15 0.516 0.643 3 5.22 0.817 0.561 Calculate the rate constant(k) for each run. Assuming the Rate Law = k[I-]2[H2O2] calculate the average rate constant,k, for this reaction. Give your answer to 2 places after the decimal.
I'(ac) + OCI (aq) 10 (aq) + Cl (aq) The rate law for the above reaction was found to be: Rate = k[I"][OCI] The Rate constant was found to be 3.7 L/mol.s Calculate the initial rate in mol/L.s for an experiment where both l and OCl are initially present at 0.73 M (Note: Write your answer to 2 d.p. e.g 1.25) Answer:
Find the half-life of CO in the presence of Ru, we need to consider the pseudo-first order reaction with the given rate law ____ Min Rate = (0.845 min^(-1)) [CO]. Step 1: CO (g) +2 Ru(s) →2 RuCO (s) Step 2: 2RuCO(s) + 3H2(g) →2 CH4(g) + 2 Ru(s)
It may not surprise you to know that products can show up in the rate law. When the product(s) is(are) a positive order, we describe the rate law as autocatalytic. For example, under conditions of high nitric acid concentrations, this reaction: HNO, + H₂C(OH): → HNO; + HCOOH + H₂O has a rate law: rate = k [H.C(OH).] [HNO₂] Given a rate constant of 0.0255 dm3 mol-1 s-1 and initial concentrations [HNO,] = 5.0 mol dm-3, [H.C(OH).]. = 150 mmol dm-3, [HNO:]. = 8.2 mmol dm-3, how long will it take for the methanediol concentration to fall to 52 mmol dm-3?
Given the following kinetic data for the first order production of H2O2, what is the rate constant (k) for the reaction? Do not put units in your answer. Trial Time (h) [H2O2] (M) ln[H2O2] 1 0 1.000 0.0 2 6.00 0.500 −0.693 3 12.00 0.250 −1.386 4 18.00 0.125 −2.079 5 24.00 0.0625 −2.772
-1 At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0482 s H,CO3 (aq) → H,O (aq)+ CO, (aq) Suppose a vessel contains H,CO, at a concentration of 0.300M. Calculate how long it takes for the concentration of H,CO, to decrease by 88.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. S x10
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