The reaction between nitrogen dioxide and carbon monoxide is NO2(g) + CO(g) → NO(g) + C02(g) The rate constant at 701 K is measured as 2.57 M-'. s measured as 567 M¯'.s The activation energy is 1.5 x and that at 895 K is 102 kJ/mol. Predict the rate constant at 525 K. Express your answer in liters per mole-second to three significant figures. Templaes Symbols uado redo reset keyboard shortcuts help, mol·s Request Answer Submit

Chemistry by OpenStax (2015-05-04)
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Chapter12: Kinetics
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Problem 63E: Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value...
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The reaction between nitrogen dioxide and carbon monoxide is
NO2(g) + CO(g) → NO(g) + C02(g)
The rate constant at 701 K is measured as 2.57 M-'. s
measured as 567 M¯'.s The activation energy is 1.5 x
and that at 895 K is
102
kJ/mol.
Predict the rate constant at 525 K.
Express your answer in liters per mole-second to three significant figures.
Templaes Symbols uado redo reset keyboard shortcuts help,
mol·s
Request Answer
Submit
Transcribed Image Text:The reaction between nitrogen dioxide and carbon monoxide is NO2(g) + CO(g) → NO(g) + C02(g) The rate constant at 701 K is measured as 2.57 M-'. s measured as 567 M¯'.s The activation energy is 1.5 x and that at 895 K is 102 kJ/mol. Predict the rate constant at 525 K. Express your answer in liters per mole-second to three significant figures. Templaes Symbols uado redo reset keyboard shortcuts help, mol·s Request Answer Submit
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