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11 Nov 2019
of the Arrhenius Equation 28 of 30 Part A The reaction between nitrogen dioxide and carbon monoxide is NO2 (g) + CO(g) â NO(g) + CO2 (g) The rate constant at 701 K is measured as 2.57 M-1-8-1 and that at 895 K is measured as 567 M1.s-1. The activation energy is 1.5Ã102 kJ/mol. Predict the rate constant at 525 K Express the rate constant in liters per mole-second to three significant figures. mol-s Submit Request Answer nrt sc f9
of the Arrhenius Equation 28 of 30 Part A The reaction between nitrogen dioxide and carbon monoxide is NO2 (g) + CO(g) â NO(g) + CO2 (g) The rate constant at 701 K is measured as 2.57 M-1-8-1 and that at 895 K is measured as 567 M1.s-1. The activation energy is 1.5Ã102 kJ/mol. Predict the rate constant at 525 K Express the rate constant in liters per mole-second to three significant figures. mol-s Submit Request Answer nrt sc f9
Collen VonLv2
28 Jan 2019