The activation energy of a certain reaction is 50.0 kJ/mol . At 23 ∘C , the rate constant is 0.0150s−1. At what temperature in degrees Celsius would this reaction go twice as fast? Express your answer with the appropriate units   B) Given that the initial rate constant is 0.0150s−1 at an initial temperature of 23 ∘C , what would the rate constant be at a temperature of 110. ∘C for the same reaction described in Part A? Express your answer with the appropriate units.

The reaction: C4H8(g)⟶2 C2H4(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1×10−8 s−1. What is the value of the rate constant at 860.0 K?

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At A reaction of A products follow a second constant of 3.76 X65M's, order → Kinetics with a

Consider the hypothetical reaction: 2 X + Y → 2 Z and its general rate law: Rate = The following data were obtained when the reaction was studied at 660 K: k[X][Y]n [X], M 0.010 0.020 0.010 [Y], M 0.010 0.010 0.020 (a) What is the order of reaction with respect to X? (b) What is the order of reaction with respect to Y? (c) What is the overall order of reaction? (d) What is the rate law? (e) What is the value of the rate constant? (2 points) (2 points) (1 point) (1 point) (2 points) Rate, M/s 2.5 x 10-5 1.0 x 10-4 5.0 x 10-5 (f) What is the rate of the reaction if [X] =0.015 M and [Y] =0.005 M? (2 points)

A particular first-order reaction has a rate constant of 1.35 x 102 s at 25.0 ° C. What is the magnitude of k at 55.0°C if Ea = 55.5 kJ/mol. 1.05 103 2.67 1065 277 1.35 102 1.65 104

Consider the reaction: 2NO(g) + O₂(g) 2 NO₂ (g) Suppose that a particular moment during the reaction nitric oxide (NO) is reacting at a rate of -0.054 M S

3. The following mechanism is proposed for the reaction of chlorine with chloroform: Cl, + CHCI, CCI, + HCI Cl, Step 1 fast equilibrium 2Cl CHCI, +CI » HCI +CCI, CCI, +Cl»cCI, Step 2 slow Step 3 fast a) Show that this mechanism gives the correct, overall balanced reaction equation. b) Write the rate law predicted by this mechanism.

The rate constant of a reaction is 5.70x10^-5 L/molxs at 195 degrees Celsius and 4.15x10^-3L/molxs at 258 degrees Celsius. What is the activation energy of the reaction? Be sure to use correct significant figures.