We're being asked to determine which among the statements are incorrect.
Recall that the rate law only focuses on the reactant concentrations and has a general form of:
k = rate constant
A & B = reactants
x & y = reactant orders
Given reaction: aA + bB + C → dD + eE
Rate Law: Rate = k[A]q[B]r[C]s
Analyzing each given statement:
Consider the reaction
aA + bB + C → dD + eE
The rate law is known to be
Rate = k[A]q[B]r[C]s
Which of the following statements is incorrect?
A) The exponents q and r are always equal to the coefficients a and b, respectively.
B) The overall reaction order is q + r + s.
C) The exponent s must be determined experimentally.
D) The symbol k represents the rate constant.
E) The exponents q, r, and s are sometimes non-integers.
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