Question

At 40 C H2O2(aq) will decompose according to the following reaction:

2H2O2 (aq) -----> 2H2O (l) + O2 (g)

The following data were collected for the concentration of H2O2 at various times:
Time (s) H2O2 (mol/L)
1.000 2.16 x 10^4
0.500 4.32 x 10^4

(a) calculate the average rate of decomposition of H2O2 between0 and 2.16 x 104 s. Use this rate to calculate the averagerate of production of O2 (g) over the same time period.
(b) what are these rates for the time period 2.16 x 104 s to4.32 x 104 s ?

Answer 1

Answer:

a. 1,157x10⁻⁵M/s

b. 5,787x10⁻⁶M/s

Explanation:

For the reaction:

2H₂O₂(aq) → 2H₂O(l) + O₂(g).

a. The rate law of descomposition is:

$rate=-\frac{1}{2} \frac{d[H_{2}O_{2}]}{dt}=\frac{d[O_{2}]}{dt}$

Where d[H₂O₂] is the change in concentration of H₂O₂ (between 0s and 2,16x10⁴s) is (1,000M-0,500M) and dt is (0s-2,16x10^4s). Replacing:

$rate=-\frac{1}{2} \frac{0,500M}{-2,16x10^4s}$

$rate=1,157x10^{-5}M/s$

As this rate is = d[O₂]/dt(Rate of production of O₂), the rate of production of O₂(g) is 1,157x10⁻⁵M/s

b. Between 2,16x10⁴s and 4,32x10⁴s, rate law is:

$rate=-\frac{1}{2} \frac{0,500M-0,250M}{2,16x10^4s-4,32x10^4s}$

$rate=5,787x10^{-6}M/s$

The rates are 5,787x10⁻⁶M/s

I hope it helps!

Answer 2

The study of chemicals and bonds is called chemistry. There are two types of elements these rare metals and nonmetals.

Thus the rate is,

$rate=1157\times10^{-5}$

What is rate law?

The rate law or rate equation for a chemical reaction is an equation that links the initial or forward reaction rate with the concentrations or pressures of the reactants and constant parameters.

The balanced reaction is:-

$2H_2O_2(aq)----->2H_2O(l)+o_2(g)$

The rate law of decomposition:-

$rate=-\dfrac{1}{2}\dfrac{d[H_2O_2]}{dt}$

Where d[H₂O₂] is the change in concentration of H₂O₂ (between 0s and 2,16x10⁴s) is (1,000M-0,500M) and dt is (0s-2,16x10^4s). Replacing:

$rate=-\dfrac{1}{2}\dfrac{0.5}{2.16\times10^{4}}$

$rate=1157\times10^{-5}$

As this rate is = d[O₂]/dt(Rate of production of O₂), the rate of production of O₂(g) is 1,157x10⁻⁵M/s

For more information about the rate of reaction, refer to the link:-

brainly.com/question/16759172