A + 2 B = C + D describes an elementary reaction, which takes place in a single step. Thus, the rate law must be
a) rate = k (A)^2
b) rate = k (B)^2
c) rate = k (A) (B)
d) rate = k (A) (B)^2
I think its D because there are 2 moles of B and 1 mole of A. Do you agree with my answer, if not please explain to me why. Thank you
Based on the given balanced chemical equation A + 2B = C + D, we can determine the rate law by examining the stoichiometry of the reaction. The stoichiometry tells us how the reactants are involved in the reaction and how they are related to the rate of the reaction.
In this case, the stoichiometric coefficients in the balanced equation tell us that for every one mole of A, two moles of B are involved in the reaction. This suggests that both A and B are reactants and contribute to the rate of the reaction.
Now let's consider the options:
a) rate = k (A)^2
This option assumes that the reaction rate is only dependent on the concentration of A, but it neglects the role of B.
b) rate = k (B)^2
This option assumes that the reaction rate is only dependent on the concentration of B, but it neglects the role of A.
c) rate = k (A) (B)
This option correctly takes into account both A and B as reactants and suggests that the reaction rate is directly proportional to the concentrations of A and B.
d) rate = k (A) (B)^2
This option suggests that the reaction rate is proportional to the concentration of A and the square of the concentration of B. However, based on the stoichiometry of the reaction, there is no indication that B is involved with a square factor.
Based on the above analysis, the correct answer would be c) rate = k (A) (B), because both A and B are reactants and contribute to the rate of the reaction in a linear fashion.