Enter your answer in the provided box. The variation of the rate constant with temperature for the first-order reaction 2N205(g) 2N204(g) + 02(g) is given in the following table. Determine graphically the activation energy in kJ/mol for the reaction. T(K)k(s1) 298 1.74 x 10-5 308 6.61 x 10 318 2.52 x 10 328 7.59 x 10 338 2.40 x 10-3 kJ/mol

The rate constant of the elementary reaction C4H8 (9)→2C2H₁ (9) is k=1.23 x 10 s¹ at 427 °C, and the reaction has an activation energy of 261 kJ/mol. Compute the rate constant of the reaction at a temperature of 464 °C. k= 8 Values if needed for this question. At a temperature of 427 °C, 5.64 x 10³ s is required for half of the C4H8 originally present to be consumed. How long will it take to consume half of the reactant if an identical experiment is performed at 464 °C? t= S

The rate constant for the reactionBr(g)+O3​(g) --> BrO(g)+O2​(g)was determined at the four temperatures shown in the table below.  T (K) k [cm3/(molecule•s) 238 5.90 x 10-13 258 7.70 x 10-13 278 9.60 x 10-13 298 1.20 x 10-12 Plot the above data, and then use that data to calculate the activation energy for this reaction.

How long will it take for the concentration of A to decrease from 1.25 M to 0.289 for the second-order reaction A → Products? (k = 1.52 M⁻¹min⁻¹)