Consider the gasphase reaction between nitric oxide and bromine at
273 ∘C 2NO(g)+Br2(g)→2NOBr(g). The following data for the initial rate of appearance of NOBr were obtained:

Part D What is the rate of disappearance of Br2 when [NO]= 7.6×10^{−2} M and [Br2]=0.21 M ? Please help with part d! 
Let the rate (r) = K[ NO]^{m} [Br2]^{n}
m and n are orders with respect to [NO] and [Br2] respectively
from experiment 1
24= K[0.1]^{m} [0.2]^{n} (1)
From experiments 2
150= K[0.25]^{m} [0.2]^{n} (2)
Eq.2/ Eq.1 gives (2.5)^{m}= 6.25 , m=2
From experiment 3
60= K[0.1]^{m} [0.5]^{n} (3)
Eq.3/ Eq.1 gives 60/24= (0.5/0.20)n, 2.5= 2.5^{n}, n=1
The rate becomes –r= K[[NO]^{2} [Br]^{1}
From Eq.1 24= K[ 0.1]^{2} [0.2]^{1}
K=12000 /M2.sec
So the rate becomes –r = 12000[ NO]^{2} [Br]^{1}
The validity of this equation for experiments 4 is also verified.
when [NO] =7.6*102 M and [Br2]=0.21M
Rate r =12000*[7.6/100)2 [0.21]=14.55 M/s
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