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Given the following reactionCH3NNCH3(g) ==> C2H6(g) + N2(g)and the measured kinetic data below: [ CH3NNCH3(g) ] MRate M/s0.01132.86 x 10-60.02261.28 x 10-5 what is the order with respect to (each of the) reactants CH3NNCH3(g),?Type your calculated answer for CH3NNCH3(g) here:

Question

Given the following reaction

CH3NNCH3(g) ==> C2H6(g) + N2(g)

and the measured kinetic data below:

 

[ CH3NNCH3(g) ] M Rate M/s
0.0113 2.86 x 10-6
0.0226 1.28 x 10-5

 

what is the order with respect to (each of the) reactants CH3NNCH3(g),?

Type your calculated answer for CH3NNCH3(g) here:

check_circleAnswer
Step 1
  • The rate law of a reaction expresses the relationship between the concentration of the reactant species and the rate of that chemical reaction.
  • And Order is equal to the sum of the exponents of the concentration of reactant species in the rate law.
For example
A+2B+C D
Rate [A[B
. Rate k [A] [B]
where k is the rate constant
and
order of this reaction = 3
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For example A+2B+C D Rate [A[B . Rate k [A] [B] where k is the rate constant and order of this reaction = 3

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Step 2

For the given reaction , let the order of reaction with respect to CH3NNCH3 be x. Therefore Rate law can be written as-

Rate = k[CH3NNCH3]m where k is the rate constant.

CH,NNCH (g)>C,H(g)+N2(g)
Rate k[CH NNCH ]
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CH,NNCH (g)>C,H(g)+N2(g) Rate k[CH NNCH ]

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Step 3

The given data is -

[CH3NNCH3], M

Rate M/s

0.0113

2.86 x 10-6

0.0226

1.28 x 10-5

Thus we can write two different equations for rate law and then evaluate them to determine the value of order of th...

Rate 1= 2.86 x 10= k[0.0113]|
Rate 2= 1.28x10-k[0.0226]
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Rate 1= 2.86 x 10= k[0.0113]| Rate 2= 1.28x10-k[0.0226]

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