The rate constants for the first order reaction 2 A - 2 8 + Cwere found at different temperatures (below). What is the activation energy for this reaction in k/mol?T1 = 17 °ck1 = 0.405T2 = 67 °Ck2 = 16.1Report your answer the nearest whole numberk2In-R T2k = Ae%3B

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Answered: The rate constants for the first order…

Chemistry

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

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Physical chemistry
Using the data in the table, calculate the rate constant of this reaction. k= A+B C+D Trial 1 2 3 Units [A] (M) 0.260 0.260 0.364 [B] (M) 0.350 0.945 0.350 Rate (M/s) 0.0167 0.122 0.0234
The activation energy for the following first-order reaction is 102 kJ/mol. N205(9) → 2NO2(g) + '½02(g) The value of the rate constant (k) is 1.35 × 104sat 35°C. What is the value of k at 0°C? Multiple Choice 1.9 x 10-5 5-1 8.2 x 10-7s-1 22x 10-25-1 4.2x 10-5-1
How would you find the rate law for this question?
Q2) Consider the following third order reaction: A➜ product The following is the integrated rate law for the third order reaction: 2[A];² 11/2 = kt + 1.5 K[A]0² 2[A]o² If the concentration of the reactant after 26.5 second of the experiment was found to 0.348 M and the rate constant for this reaction was found to be 1.5x10¹² M².S¹. a) Determine the initial concentration of the reactant. b) What is the half-life of this reaction? c) What is the concentration of the reactants after 1.00 min of the experiment?
r = L [A] [B] ² x2 x 2 r=k [2A) [21] ² 8x bigger than 2 + 4 = 8 12. Consider a reaction of the form 2A + BC. The data for this reaction is given below: Initial rate of formation of C M/s Initial [A] Initial [B] 4.0 x 10-² 0.30 0.10 2.0 x 10-² 0.50 0.05 6.0 x 10-² 0.50 0.15 1.0 x 10-² 0.025 a. What rate law is consistent with this data? 0.40 b. Calculate k and specify units. How long will it take for the concentration of C to equal to 0.10 molar if the initial concentration of all the species are [A] = 0.4 M, [B] = 0.3 M and [C] = 0.0 M?
The gas-phase reaction 2 N₂O5 (g) → 4 NO₂ (g) + O2 (g) has an activation energy of 103 kJ/mol, and the rate constant is 0.0900 min-1 at 328.0 K. Find the rate constant at 313.8 K. The value of gas constant is 8.3145 × 10-³ kJ/K - mol. Rate constant = min-1
See image below. Can you please show me how to solve this?
The rate constant for the reaction of nitrogen with oxygen was determined at four temperatures. N2(g) + O2(g) T(K) 2NO(g) k (cm3/molecule⚫s) 250 7.18 x 10-8 275 1.36 x 10-7 300 2.31 x 10-7 325 3.46 x 10-7 3rd attempt Part 1 (1 point) Plot these data to calculate the activation energy of the reaction. kJ/mol Part 2 (1 point) Plot these data to calculate the frequency factor A for the reaction. cm3/molecules
4
A student runs two different reactions, whose energy diagrams are graphed below on the same scale. Which relationships concerning the activation energies of the two reactions (E3(1) and E,(2) and the rate constants of the two reactions (k1 and k2) are correct? Reaction 1 Reaction 2 Reaction coordinate Reaction coordinate Ea(1) > Ea(2) k1 > k2 Ea(1) > Ea(2) k1 k2 Ea(1) < Ea(2) k1 < k2 Energy Energy

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The rate constants for the first order reaction 2 A - 2 8 + Cwere found at different temperatures (below). What is the activation energy for this reaction in k/mol? T1 = 17 °c k1 = 0.405 T2 = 67 °C k2 = 16.1 Report your answer the nearest whole number k2 In- R T2 k = Ae %3B