Problem: Consider the reactionaA + bB + C → dD + eEThe rate law is known to beRate = k[A]q[B]r[C]sWhich 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.

FREE Expert Solution

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:

rate law=kAxBy

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:

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Problem Details

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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