uovelei lottivity.doriocator.assignment-take&takeAssignmentSessionLocator;=assig

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uovelei lottivity.doriocator.assignment-take&takeAssignmentSessionLocator;=assignment-take Use the References to access important values if needed for this question. The oxidation of nitrogen monoxide by oxygen at 25 °C 2 NO +02 +2 NO2 is second order in NO and first order in 02 Complete the rate law for this reaction in the box below. not appear. Use the form kIA)[B!"., where 'l' is understood for m, n... don't enter I) and concentrations taken to the zero power do Rate In an experiment to determine the rate law, the rate constant was determined to be 1.05x10 Mr',-1.Using this value for the rate constant, the rate of the reaction when [NO]-8.80x103 M and [O2]-2.96x103 M would be Ms. 9 more group attempts remaining Retry Entire Group

Explanation / Answer

The given reaction is : 2NO + O2 ----> 2NO2

The above reaction is second order in NO and first order in O2.

Therefore, rate = k[NO]2[O2]

Again,

k = 1.05 x 104 M-2s-1 , [NO] = 8.80 x 10-3 M, [O2] = 2.96 x 10-3 M

Now , rate =  k[NO]2[O2]

=> rate = 1.05 x 104 M-2s-1 x (8.80 x 10-3 M)2 x  2.96 x 10-3 M

=> rate = 240.68352 x 10-5 Ms-1 = 2.41 x 10-3 Ms-1

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