For the reaction show below determine the rate law. H2SO3(aq) + 6I-(aq) + 4H+(aq) → S(s) + 2I3- + 3H2O (l) In the presence of a
little starch, this solution turns from colorless to blue when I3- is formed. The following data were obtained: [H2SO3] [H+] [I-] Initial Rate (mol/L s) 1.0 x 10-2 2.0 x 10-1 2.0 x 10-1 1.66 x 10-7 3.0 x 10-2 2.0 x 10-1 2.0 x 10-1 4.98 x 10-7 1.0 x 10-2 1.0 x 10-1 2.0 x 10-1 8.30 x 10-8 1.0 x 10-2 2.0 x 10-1 4.0 x 10-1 13.2 x 10-7 Calculate the rate law for this reaction: rate = k [H2SO3] [H+] [I-
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In the electrolysis of water, 3490 hour will it take to produce 165.0 L of H2 at 1.0 atm and 273 K using an electrolytic cell through which the current is 113.0 mA.
<h3>What is Ideal Gas Law ?</h3>The ideal gas law states that the pressure of gas is directly proportional to the volume and temperature of the gas.
It is expressed as
PV = nRT
where,
P = Pressure
V = Volume in liters
n = number of moles of gas
R = Ideal gas constant
T = Temperature in kelvin
Here,
P = 1.0 atm
V = 165.0 L
R = 0.0821 atm. L/mol.K (Ideal gas constant)
T = 273 K
n = ?
Now put the value in above expression, we get
PV = nRT
1.0 atm × 165.0 L = n × 0.0821 atm. L/mol.K × 273 K
165.0 atm. L = n × 22.4 atm. L/mol
n = 7.36 mol
The reaction is
2H⁺ + 2e⁻ → H₂
1 mol of electrons is produced from 96500 C
So,
<em>= </em>1,420,480 C
<u>Convert milliampere to C/s</u>
1mA = 0.001 C/s
113.0 mA = 113.0 × 0.001
= 0.113 c/s
<h3>What is relationship between current, charge and time ?</h3>The relation between current, charge and time is expressed as:
where,
I = Current
Q = Charge in Coulomb
t = time
Now put the value in above formula we get
= 12,570,619.469 s
= 3490 hour
Thus from the above conclusion we can say that In the electrolysis of water, 3490 hour will it take to produce 165.0 L of H2 at 1.0 atm and 273 K using an electrolytic cell through which the current is 113.0 mA.
Learn more about the Ideal Gas Law here: brainly.com/question/25290815
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