Constants | Periodic Table Part A The reaction between nitrogen dioxide and carb

Question

Constants | Periodic Table Part A The reaction between nitrogen dioxide and carbon monoxide is Use the value of the activation energy (Ea-1.50 × 102 kJ/mol) and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 564 K. NO2 (g) + CO(g) NO(g) + CO2 (g) The rate constant at 701 K is measured as 2.57 M-1.s-1 and that at 895 K is measured as 567 M1s-1 M-1s1 You may want to reference (Pages 606- 612) Section 14.6 while completing this problenm Submit Request Answer

Explanation / Answer

at temperature = 701 K and rate constant(K2) = 2.57 M-1S-1.

at temperature = 564 K and rate constant = K1 M-1S-1.

Ea = 1.50 * 10^2 KJ / mole = 1.50 * 10^5 J/mole.

we know,

ln (K2 / K1) = Ea /R * (T2 - T1) / T1T2

ln (2.57 / K1) = 1.50 * 10^5 / 8.314 * (701 - 564) / 564 * 701

ln (2.57 / K1) = 6.25

2.57 / K1 = 518

K1 = 4.96 * 10^-3 M-1 S-1

so rate constant at 564 K is 4.96 * 10^-3 M-1 S-1

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