2A-B+C Two trials of the above reaction are run with the same initial concentration of A The first trial is performed at 25°C and the second at 35°C. IH the rate constant at 25°C is 0.579 M/min, what is the rate constant in the second trial if the reaction has an activation energy of 31 3 kJ/mol?

1.) Consider the reaction below at 100°C T2U (g) --> 2T(g) + U (g) When [T2U], is 0.250 M, the reaction rate is 9.30 x 10³ M/s, and when [T2U], is 0.144 M, the reaction rate is 3.09 x 103 M/s. If the reaction has an activation energy of 66 kJ/mol, what is the numerical value of the rate constant at 25°C?! A. 0.000703 B. 0.00472 С. 0.0373 D. 0.117

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The activation energy of an uncatalyzed reaction is 86 kJ/mol. The addition of a catalyst lowers the activation energy to 61 kJ/mol Part A Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 24 °C? Express the ratio to two significant digits. ke/ku = 2.2 • 1o Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Part B Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 128 °C? Express the ratio to two significant digits. ? ke/k, = 2.9 • 10² Submit Previous Answers Request Answer X Incorrect; Try Again; 8 attempts remaining

3. You have a reaction that is run at 273°C and has a rate constant of 2.52 x 10/s. The same reaction is run at 157 °C and has a rate constant of 1.0 x 10-/s. What is the activation energy for this reaction? (R = 8.314 J/mol K) %3D 0.00898mols 102 sec 4. w for ate= k[NO2]?. The rate constant for this reaction: If yo tion for 5 minutes urd be the concentra

(Arrhenius equation); I’m not sure what the molecular collision constant (A) would be

For the multi-step reaction A +B C+D the rate-limiting step is unimolecular, with A as the sole reactant. If [A] and [B] are both 0.110 M, then the rate of reaction is 0.0020 M/s. What is the rate of the reaction if [A] is doubled? rate: M/s Starting with the original concentrations, what is the rate of the reaction if [B] is doubled? rate: M/s Starting with the original concentrations, what is the rate of the reaction if [A] and [B] are both increased by a factor of 3? rate: M/s

Aktiv Chemistry C https://app.101edu.co Dib X + O Question 15 of 15 The activation energy, Ea, for a particular reaction is 19.4 kJ/mol. If the rate constant at 80 °C is 0.820 M¹s 1, then what is the value of the rate constant at 215 °C? (R = 8.314 J/mol K)

The rate constant for the reaction below at 701K is 2.57 M-1s-1.NO2 (g) + CO (g) → NO (g) + CO (g)Calculate the rate constant at 895K given the activation energy to be 145 kJ/mol.

The proposed mechanism for a reaction is 1. A(g) + B(g) ⇄ X(g) Fast 2. X(g) + C(g) ⇄ Y(g) Fast 3. Y(g) → D(g) Slow Which of the following would be a rate law for the reaction? *The answer is: rate = k[A][B][C], but i would like an explanation*