What is the value of the rate constant for this reaction at this temperature?
The frequency factor is #7.50 xx 10^12 "M"^(-1)cdot"s"^(-1)# , the activation energy is #"62.0 kJ/mol"# , and the temperature is #24.0^@ "C"# .
The frequency factor is
1 Answer
Oct 5, 2017
#k = "94.8 M"^(-1)"s"^(-1)#
The relation between the rate constant and temperature is something you should be getting to know really well at this point:
#k = Ae^(-E_a//RT)# (what is the equation called?)
#k# is the rate constant.#A# is the frequency factor, which has the same units as the rate constant.#E_a# is the activation energy, usually in#"kJ/mol"# .#R = "0.008314472 kJ/mol"cdot"K"# is the universal gas constant that ensures the units cancel in the exponential.#T# is the temperature in#"K"# .
And so this is mostly plugging it in and using a calculator.
#color(blue)(k) = 7.50 xx 10^12 "M"^(-1)"s"^(-1) cdot e^(-"62.0 kJ/mol"/("0.008314472 kJ/mol"cdot"K" cdot (24.0 + "273.15 K"))#
#= (7.50 xx 10^12) e^(-25.095) "M"^(-1)"s"^(-1)#
#=# #ulcolor(blue)("94.8 M"^(-1)"s"^(-1))#
What is the order of this reaction?
