Hi there, I have the answers for the question below but I want how to solve step

Question

Hi there,

I have the answers for the question below but I want how to solve step by step

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Thanks in advance

16. The rate constant for the reaction 2NO2 N204 is 2.79 L/mol-min at 48°C. If the initial concentration of NO2 is 1.05 M, what is the half-life? a. 10.3s b. 0.341 s c. 176s 14.9 s e20.5 s 17.-Given the following data for the NH4+ + NOg N2 + 2H2O reaction Trial 0.010 M 0.015 0.010 O, 0.020 M 0.020 0.010 Rate 0.020 M/s 0.030 0.005 The rate law for the reaction is rate =k[NH4+][NO2-p rate = k[NH4+][NO2.] rate = k[NH4+]2[NO,-] rate = k[NH4+]2[N0212 None of the above b. c. d. e. 18. The specific rate constant, k, for a reaction is 0.44 s1 at 25 °C, and the activation energy is 245 kJ/mol. Calculate k at 125 °C. (The universal gas constant 8.314 J/mol-K.) a. 8.32 x 10 s b. 1.03×1010 s-1 2.71 x 1010s 4.51 × 10's!

Explanation / Answer

16)

Given:

k = 2.79 L/mol.min

By seeing the unit of k, this is 2nd order reaction

use relation between rate constant and half life of 2nd order reaction

t1/2 = 1/([NO2]o*k)

= 1/(1.05*2.79)

= 0.3414 min

= 0.3414*60 s

= 20.5 s

Answer: e

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