Chemistry - Chemical Kinetics Question with Solution | TestHub
The reaction between A and B is of first order with respect to A and of zero order with respect to B. The following data was obtained for four experiments
The value of is
Options:
Answer:
Solution:
A. Question Explanation:
The question provides experimental data for a reaction between A and B , where the reaction is first order with respect to A and zero-order with respect to B . You need to use this information to determine the values of , and z in the table.
B. Concept: Rate law
Solution -
Rate Law: For a reaction with rate = k[A]m [B]n , where m and n are the orders with respect to A and B, respectively.
First-Order Reaction: Rate = k[A] (since the order with respect to A is 1).
Zero-Order Reaction: Rate is independent of [B] (since the order with respect to B is 0).
D. Mathematical Calculation:
1. Write the Rate Law:
Since the reaction is first-order in A and zero-order in B, the rate law is:
Rate = k[A]
2. Find the Rate Constant (k) using Experiment I:
2.5 × 10-2 M/min = k × 0.15 M
k = (2.5 × 10-2 M/min) / 0.15 M
k = 0.1667 min-1
3. Find x using Experiment II:
3.75 × 10-2 M/min = k x
3.75 × 10-2 M/min = 0.1667 min-1 x
x = (3.75 × 10-2 M/min) / 0.1667 min-1
x = 0.225 M
4. Find y using Experiment III:
y = k × 0.135 M
y = 0.1667 min-1 × 0.135 M
y = 0.0225 M/min
y = 2.25 x 10-2 M/min
5. Find z using Experiment IV:
3.75 × 10-3 M/min = kz
3.75 × 10-3 M/min = 0.1667 min-1 z
z = (3.75 × 10-3 M/min) / 0.1667 min-1
z = 0.0225 M
E. Final Answer:
x = 0.225 M
y = 2.25 × 10-2 M/min
z = 0.0225 M