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Part A Consider the following reaction: A+B+C->D The rate law for this reaction is as follows: Rate =k([A][C]^(2))/([(B)]^((1)/(2))) Suppose the rate of the
Part A\ Consider the following reaction:\
A+B+C->D
\ The rate law for this reaction is as follows:\ Rate
=k([A][C]^(2))/([(B)]^((1)/(2)))
\ Suppose the rate of the reaction at certain initial concentrations of
A,B
, and
C
is
1.14\\\\times 10^(-2)(M)/(s)
.\ What is the rate of the reaction if the concentrations of
A
and
C
are doubled and the concentration of
B
is tripled?\ Rate
2=
\
(M)/(s)
\ Previous Answers\ Request Answer
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