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Henry's law Quiz

Henry's law  Quiz

Henry's law Quiz Test "How well do you understand the laws in chemistry? Although it is not an easy subject to remember. The thing I believe, more or less you are familiar with the terms Henry's law. In this quiz, we are going to face some of the very common and important quizzes which you have witnessed before. Because Henry's Law is one of the most often used, and misused, principles of physical chemistry. Its application extends to many branches of science and engineering where the solubility of gases in liquids is an important phenomenon. Let’s look back at the history of this law. The law was first formulated in 1803 by the English physician and chemist William Henry. Henry’s law defines that at a constant temperature, the concentration of the gas that is dissolved in a given liquid is proportional to the partial pressure of the gas above the fluid. In his publication about the number of gases absorbed by water, he described the results of his experiments: ""water takes up, of gas condensed by one, two, or more additional atmospheres, a quantity which, ordinarily compressed, would be equal to twice, thrice, &c. the volume absorbed under the common pressure of the atmosphere."" The equation is C=kPgas. Where, C is the solubility of a gas at a fixed temperature in a particular solvent (in units of M or mL gas/L) k is Henry's law constant (often in units of M/atm) Pgas is the partial pressure of the gas (often in units of atm) "

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Quiz Questions And Answers

Solubility of a gas in a liquid is directly proportional to:

Volume of the gas
Pressure of the gas
Temperature of the gas
Gas constant

Density of a 2.05 M solution of acetic acid in water is 1.20 g/mL. The molarity of the solution is:

3.28 mol kg-1
2.28 mol kg-1
0.44 mol kg-1
2.14 mol kg-1

Aquatic species are more comfortable in cold water than that of warm water because:

Solubility of O2 increases with increase in Pressure
Solubility of O2 decreases with increase in Pressure
Solubility of O2 increases with increase in Temperature
Solubility of O2 decreases with increase in Temperature

Which best describes the solid in gas solution:

Camphor vapours in nitrogen gas
Chloroform vapours mixed with nitrogen gas
Solution of hydrogen in palladium
Oxygen dissolved in water

What would be the molarity of the aqueous solution if 36 g glucose (molar mass, 180 g mol-1) is present in 750 cm3 of aqueous solution:

0.367 M
0.267 M
0.167 M
0.067 M

A mixture of acetone with chloroform show:

Shows a positive deviation from Raoult’s Law
Behaves like a near ideal solution
Follows Henry’s Law
Shows negative deviation from Raoult’s Law

At what temperature will water boil, if 54 g of glucose, C6 H12 O6 is dissolved in 1 kg of water. The value of Kb for water is 0.52 K kg mol-1.

373.202 K
373.15 K
373.306 K
373.216 K

The solid and the liquid are in equilibrium at:

The boiling point of the solute
The freezing point of the solvent
The freezing point of the solution
The freezing point of the solute

What would be the molar mass of the solute, if 10 g of a non-electrolyte solute is dissolved in 100 g of benzene which lowered the freezing point of benzene by 0.50 K.

2104 g mol-1
2104 g mol-1
1042 g mol-1
1024 g mol-1

Solutions having same osmotic pressure are called:

Solutions having same osmotic pressure are called:
Isochoric solutions
Isotonic solutions
None of the above

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