Question

* WORTH 30 POINTS + BRAINLIEST *

The table shows the rate of reaction for two unknown time intervals during the course of a reaction.


Reaction Rates
Time Intervals (s) Rate (M/s)
T1 1.1 × 10−3
T2 1.5 × 10−3

Which of the following is true for the two time intervals?

A. T1 is longer than T2, and the concentration of reactants at the end of T1 is lower than that of T2.

B. T1 is longer than T2, and the concentration of products the end of T1 is lower than that of T2.

C. T1 is shorter than T2, and the concentration of reactants at the end of T1 is higher than that of T2.

D. T1 is shorter than T2, and the concentration of products at the end of T1 is higher than that of T2.

Answer 1

Answer:

C D

Explanation:

T1) 1.1 * 10 - 3 = 8

T2) 1.5 * 10 - 3 = 12

Answer 2

Answer:

B. T1 is longer than T2, and the concentration of products the end of T1 is lower than that of T2.

Explanation:

Consider a hypothetical reaction:

A → B

The rate of the reaction can be expressed as in terms of the rate of disappearance of reactant (-dA/dt) or appearance of product (dB/dt)

$Rate = -\frac{d[A]}{dt} = \frac{d[B]}{dt}$

Here dt is the time interval

dA = change in reactant concentration [A(final) - A(initial)]

dB = change in product concentration [B(final)-B(initial)]

It is given that:

At time interval T1, Rate(1) = 0.0011 M/s

At time interval T2, Rate(2) = 0.0015 M/s

Here, Rate (2) > Rate (1): this implies that the denominator for Rate(2) is smaller than Rate (1) i.e. T2 is smaller than T1. Since the rate of conversion is smaller at T1 this implies that the concentration of products will be lower at T1 than at T2.