Part B: The rate of the reaction in terms of the \"appearance of product\" inclu
ID: 858690 • Letter: P
Question
Part B: The rate of the reaction in terms of the "appearance of product" includes the change in the concentration of the product, the time interval, and the coefficient of the product. Consider the following reaction: 2A+3B->3C+2D.
The concentrations of product C at three different time intervals are given. Use the following data to determine the rate of reaction in terms of the appearance of product C between time = 0 s andtime = 20 s .
Part C: The rate of reaction in terms of the "rate law expression" includes the rate constant (k), the concentration of the reactants, and the orders of the reaction with respect to the different reactants.
Consider the following reaction:
A+B?C+D
The initial concentrations of the reactants A and B are 0.300 M and 0.290 M, respectively.
The rate of reaction is 0.060 M?s?1, and the orders of the reaction, with respect to reactants Aand B, are 1 and 2, respectively.
Determine the rate constant (k) for the reaction using the rate law.
Time (s) 0 20 40 [C](M) 0.000 0.0240 0.0480Explanation / Answer
PartB:
2A+3B->3C+2D.
-1/2d[A]/dt = -1/3d[B]/dt = 1/3 d[C]/dt = 1/2 d[D]/dt
d[C]/dt = 0.0240/20 = 0.0012 M/sec
rate of disappearance of A = d[A]/dt = 2/3(0.0012) = 0.0008 M/sec
rate of disappearance of B = d[B]/dt = 0.0012 M/sec.
rate of appearance of C = d[C]/dt = 0.0240/20 = 0.0012 M/sec
rate of appearance of D = d[D]/dt = 2/3(0.0012) = 0.0008 M/sec.
PartC
rate = K[A]^1 [B]^2
0.06 = K(0.3)(0.29)^2
K = 2.378 M^-2 sec^-1