The substitution of CO in Ni(CO)4 by another molecule L [where L is an electron-pair donor such as P(CH3)3was studied some years ago and led to an understanding of some of the general principles that govern the chemistry of compounds having metalâCO bonds. (See J. P. Day, F. Basolo, and R. G. Pearson: Journal of the American Chemical Society, Vol. 90, p. 6927, 1968.) A detailed study of the kinetics of the reaction led to the following mechanism:
Slow Ni(CO)4 ----> Ni(CO)3 + CO Fast Ni(CO)3 + L ----> Ni(CO)3L
1. What is the molecularity of each of the elementary reactions?
a.Molecularity of the slow step =
b.Molecularity of the fast step =
2. Doubling the concentration of Ni(CO)4 increased the reaction rate by a factor of 2. Doubling the concentration of had no effect on the reaction rate. Based on this information, write the rate equation for the reaction.
Rate= _____________
(Use k for the rate constant.)
3. The experimental rate constant for the reaction, when L= P(C6H5)3 is 9.3x10-3s-1 , is at 20 °C. If the initial concentration of Ni(CO)4 is 0.021 M, what is the concentration of the product after 1.7 minutes?
Concentration = _________________ M
The substitution of CO in Ni(CO)4 by another molecule L [where L is an electron-pair donor such as P(CH3)3was studied some years ago and led to an understanding of some of the general principles that govern the chemistry of compounds having metalâCO bonds. (See J. P. Day, F. Basolo, and R. G. Pearson: Journal of the American Chemical Society, Vol. 90, p. 6927, 1968.) A detailed study of the kinetics of the reaction led to the following mechanism:
| Slow Ni(CO)4 ----> Ni(CO)3 + CO | ||
| Fast Ni(CO)3 + L ----> Ni(CO)3L |
1. What is the molecularity of each of the elementary reactions?
a.Molecularity of the slow step =
b.Molecularity of the fast step =
2. Doubling the concentration of Ni(CO)4 increased the reaction rate by a factor of 2. Doubling the concentration of had no effect on the reaction rate. Based on this information, write the rate equation for the reaction.
Rate= _____________
(Use k for the rate constant.)
3. The experimental rate constant for the reaction, when L= P(C6H5)3 is 9.3x10-3s-1 , is at 20 °C. If the initial concentration of Ni(CO)4 is 0.021 M, what is the concentration of the product after 1.7 minutes?
Concentration = _________________ M
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