A reaction with stoichiometric equation 1/2A + B = R + 1/2S has the following rate expression –rA = 2CA 0.5 CB. What is the rate expression for this reaction if the stoichiometric equation is written as A + 2B = 2R + S?
Reaction equation: ½ A + B ====> R + ½ S
Rate of disappearance of A, -rA = k[A]0.5[B]
Can also be written as -rA = k CA0.5 CB
rate expression given for the above reaction equation = -rA = 2 CA0.5 CB.
So the rate constant, k, of the reaction = 2
If the stoichiometric equation is written as A + 2B = 2R + S
Then the rate of disappearance of A will be, -rA = k[A][B]2
Can also be written as -rA = k CA CB2
Since rate constant, k, of the reaction = 2
The rate of disappearance of A will be, -rA = 2[A][B]2
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