Please do your best to complete the question in full with as much detail as you
ID: 1006319 • Letter: P
Question
Please do your best to complete the question in full with as much detail as you can spare. It does not need to be answered quickly with a simple answer so please take you time, and thank you very much.
Method of Initial Rates, Integrated Rate Law, Arrhenius Equation
The following data were collected for the rate of disappearance of A in the reaction at 25°C:
A ----> 2 C + D
a) What is the rate law for the reaction? Use METHOD of INITIAL RATES
b) What is the Rate of Appearance of C in the second experiment?
c) What would be the effect on the rate of the reaction of tripling the concentration of A?
d) What is the value of the rate constant at 25°C? Include the units of the rate constant.
e) If [A]0 = 1.40 M, what is the half life?
f) If [A]0 = 1.40 M, how long would it take for the [A] = 0. 155 M at 25°C? Use the integrated rate law.
g) If [A]0 = 1.40 M, what would be the [A] after 0.0250 seconds at 25°C? Use the integrated rate law.
h) For this reaction, which would give a straight line? A plot of ……. Circle your answer
1/[A] vs time with the slope = -k 1/[A] vs time with the slope = k
ln[A] vs time with the slope = -k ln[A] vs time with the slope = k
[A] vs time with the slope = -k [A] vs time with the slope = k
i) For this part assume that your reaction is first order, what is the rate constant at 50°C? Ea = 42.5 kJ/mol
Experiment [A], (M) Initial Rate )M/s) 1 0.10 24 2 0.20 24Explanation / Answer
Given –dcA/dt= 24, dCC/dt= 24*2= 48 M/s
0.7= 0.14- 24*t1/2, t1/2 is half life , 24t1/2= 0.7, t1/2 =0.7/24 =0.029 sec
From Ln ( K2/24)= (42.5*1000)/8.314*(1/298-1/323)( The value of Ea= 42.5 Kj/Mol)
K2= 90.54