Question

# Consider the reaction X + Y → Z From the data in the table, obtained at...

Consider the reaction X + Y → Z From the data in the table, obtained at 360 K, (a) determine the overall order of the reaction Initial Rate of Disappearance of X (M/s) [X] (M) [Y](M) 0.053 0.10 0.50 0.127 0.20 0.30 1.02 0.40 0.60 0.254 0.20 0.60 0.509 0.40 0.30 (b) determine the initial rate of disappearance of X when the concentration of X is 0.50 M and that of Y is 0.30 M.

rate of disappearance, -r= K[X]m [y]n

m, n are ordes of reaction with respect to [X] and [Y] respectively. K is the rate constant

given 0.127= K[0.2]m [0.3]n   (1)

also given 0.509 =K[0.4]m [0.3]n   (2)

Eq.2/ Eq.1 give

0.509/0.127= [2]m

2m=4, m=2

It is mentioned 0.254 =K[0.2]m [0.6]n    (3)

Eq.3/Eq.2 gives 2= 2n

n=1

so the rate expresion becomes -r =K[X]2 [Y]1

from Eq.1   0.053= K[0.1]2 [0.5]1

K= 0.053/0.005 =10.6 /M2.s

so the rate expression becomes -r = 10.6 [X]2 [Y]

at X=0.5M and Y=0.3 M

-r =10.6 [0.5]2 [0.3] =0.795 M/s

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