Find the reaction rate law and the rate law constant for NO (g) +H2(g)-> HNO2(g)?

and your data is....

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Maddie... it always help to include all the information about a problem.

you posted this data

1 0.001 0.004 0.002

2 0.002 0.004 0.008

3 0.003 0.004 0.018

4 0.004 0.001 0.008

5 0.004 0.002 0.016

6 0.004 0.003 0.024

but didn't include any column headings. I'm going to assume this

run.. . [NO]... . [H2].. .. .rate

.1 .. ..0.001.. .0.004.. ..0.002

.2 ... .0.002... 0.004.. ..0.008

.3 .. ..0.003.. .0.004.....0.018

.4 .. ..0.004.. .0.001.. ..0.008

.5 .. ..0.004.. .0.002.. ..0.016

.6 .. ..0.004.. .0.003.. ..0.024

now we know the rate equation will be of this form

.. rate = k x [NO]^m * [H2]^n

from runs 4 to 5 we see [NO] is held constant but [H2] doubles and rate doubles

so, the exponent on H2 must be 1

.. rate = k x [NO]^m x [H2]

from runs 1 to 2, we can see [H2] is constant, [NO] doubles and rate quadruples

so the exponent on [NO] must = 2

.. rate = k * [NO]² * [H2]

now if you plug in any data point, you can calculate k

.. k = rate / ([NO]² * [H2])

.. k = (0.024M/sec) / ((0.004M)² * (0.003M)) = 5x10^5 / (M² x sec)

Few.

Wa