An experiment was undertaken to determine the effect of different liquids upon the swelling of a vulcanized sample of natural ru
bber at room temperature. It was found that the equilibrium swelling ratio of the natural rubber in carbon tetrachloride was 5.5 and in benzene it was 4.4. Given the information below determine the following parameters.
(a) The molar mass between crosslinks, Mc for the natural rubber sample.
(b) The value of the Flory-Huggins interaction parameter, x, for natural rubber in benzene.
(The density of natural rubber=910 kg M^-3; Flory-Huggins interaction parameter x for natural rubber in carbon tetrachloride=0.290; molar volume of carbon tetrachloride=97.1 x 10^-6 m^3 mol^-1; and molar volume of benzene=89.4 x 10^-6 m^3 mol^-1.)
(a) The molar mass between crosslinks, Mc for the natural rubber sample.
(b) The value of the Flory-Huggins interaction parameter, x, for natural rubber in benzene.
(The density of natural rubber=910 kg M^-3; Flory-Huggins interaction parameter x for natural rubber in carbon tetrachloride=0.290; molar volume of carbon tetrachloride=97.1 x 10^-6 m^3 mol^-1; and molar volume of benzene=89.4 x 10^-6 m^3 mol^-1.)
1 answer:
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Answer:
A)
1. Reaction will shift rightwards towards the products.
2. It will turn green.
3. The solution will be cooler..
B) It will turn green.
Explanation:
Hello,
In this case, for the stated equilibrium:
In such a way, by thinking out the Le Chatelier's principle, we can answer to each question:
A)
1. If potassium bromide, which adds bromide ions, is added more reactant is being added to the solution, therefore, the reaction will shift rightwards towards the products.
2. The formation of the green complex is favored, therefore, it will turn green.
3. The solution will be cooler as heat is converted into "cold" in order to reestablish equilibrium.
B) In this case, as the heat is a reactant, if more heat is added, more products will be formed, which implies that it will turn green.
Regards.
Answer:
474 grams of chlorine gas are present in a 150 liter cylinder of chlorine held at a pressure of 1.00 atm and 0 °C
Explanation:
An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.
The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:
P*V = n*R*T
where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas.
In this case:
- P= 1.00 atm
- V= 150 L
- n= ?
- R= 0.082
- T= 0 C= 273 K
Replacing:
1.00 atm* 150 L= n*0.08206 *273 K
Solving:
n= 6.69 moles
Being Cl= 35.45 g/mole, the molar mass of chlorine gas is:
Cl₂=2*35.45 g/mole= 70.9 g/mole
So if 1 mole has 70.9 grams, 6.69 moles of the gas, how much mass does it have?
mass= 474.321 grams ≅ 474 grams
<u><em>474 grams of chlorine gas are present in a 150 liter cylinder of chlorine held at a pressure of 1.00 atm and 0 °C</em></u>