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22 February, 00:54

The reaction between nitrogen dioxide and carbon monoxide isNO2 (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 M-1⋅s-1. The activation energy is 1.5*102 kJ/mol. Predict the rate constant at 525 K. Express the rate constant in liters per mole-second to three significant figures.

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  1. 22 February, 01:31
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    Given data

    K1 = 2.57 M-1s-1

    T1 = 701 K

    K2=?

    T2 = 525 K

    Ea = 150 kJ / mol * 1000 J * / 1 kJ = 150000 J / mol

    Formula to calculate the rate constant using the activation energy is as follows

    ln[K2/K1] = (Ea / R) * [ (1/T1) - (1/T2) ]

    where R = 8.314 J per mol. K

    lets put the values in the formula and calculate the activation energy

    ln [K2/2.57] = 150000 J per mol / 8.314 J per K. mol * [ (1/701) - (1/525) ]

    ln [K2/2.57] = - 8.628

    K2 / 2.57 = anti ln [-8.628]

    K2/2.57 = 0.000179

    K2 = 0.000179 * 2.57

    K2 = 0.00046

    Therefore rate constant at 525 K is 4.6*10^-4 L/mol. s
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