Iodine clock and chemical Equilibrium 1-For this experiment, it is important to

Question

Iodine clock and chemical Equilibrium

1-For this experiment, it is important to

a)Make the concentration of Dye large compared to that of the Bleach.

Make the temperature of all the runs the same.

c)Change the activation energy for each trial

d)Change the temperature for each trial

e)Make the concentration of Bleach large compared to that of the Dye.

---------------

2-Given the following sample data from experiments, determine the orders m and n.

Rate= k [Bleach]m [Dye]n

Run

[Bleach] M

[Dye] M

Rate (M/s)

1

.08000

.04000

22.4 x 10-3

2

.06500

.02000

3.00 x 10-3

3

.02200

.04000

0.466 x 10-3

4

.08000

.02000

5.60 x 10-3

5

.04000

.04000

2.80 x 10-3

a)m = 0 and n = 1

b)m = 1 and n = 2

c)m = 2 and n = 3

d)m = 3 and n = 4

e)m = 3 and n = 2

a)Make the concentration of Dye large compared to that of the Bleach.

Make the temperature of all the runs the same.

c)Change the activation energy for each trial

d)Change the temperature for each trial

e)Make the concentration of Bleach large compared to that of the Dye.

Explanation / Answer

1) b)make the temperature of all the runs the same

bleach+dye--->products

At a given temperature, for the above reaction , rate=k[bleach]^m [dye]^n

k=rate constant

m and n are the order of rxn with respect to bleach and dye

But at different temperature k is different ,so rate is also different.

(rate dependence on temperature is given by Arrhenius equation:

k=A exp(-Ea/RT))

Also equilibrium constant=Keq=kf/kr =rate constant for forward rxn/rate constant for reverse rxn,

Related Questions

Navigate

• Browse (All)
• Browse I
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.