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According to Henry's law, what is the relationship between the solubility of an ideal gas and its partial pressure?
According to Henry's law, what is the relationship between the solubility of an ideal gas and its partial pressure?
- The solubility of an ideal gas is inversely proportional to its partial pressure
- The solubility of an ideal gas is directly proportional to its partial pressure (correct)
- The solubility of an ideal gas is proportional to the square of its partial pressure
- The solubility of an ideal gas is independent of its partial pressure
In the context of Henry's law, what does the proportionality constant 'k' depend on?
In the context of Henry's law, what does the proportionality constant 'k' depend on?
- The identity of the gaseous solute only
- The identity of the solvent only
- The temperature of the solution only
- The identities of both the gaseous solute and solvent, and the solution temperature (correct)
If the concentration of dissolved oxygen in water exposed to a partial pressure of 150 kPa is 0.002 mol L−1, what would be the new concentration if the partial pressure is reduced to 75 kPa, assuming ideal conditions according to Henry's law?
If the concentration of dissolved oxygen in water exposed to a partial pressure of 150 kPa is 0.002 mol L−1, what would be the new concentration if the partial pressure is reduced to 75 kPa, assuming ideal conditions according to Henry's law?
- 0.002 mol L−1
- 0.0005 mol L−1
- 0.001 mol L−1 (correct)
- 0.004 mol L−1
According to Henry's law, what happens to the solubility of a gas in a liquid as the partial pressure of the gas increases?
According to Henry's law, what happens to the solubility of a gas in a liquid as the partial pressure of the gas increases?
How does an increase in temperature affect the solubility of a gas in a liquid according to Henry's law?
How does an increase in temperature affect the solubility of a gas in a liquid according to Henry's law?
What is the relationship between the Henry’s law constant and the solubility of a gas in a liquid?
What is the relationship between the Henry’s law constant and the solubility of a gas in a liquid?
Why are supersaturated solutions of most solids in water prepared by cooling saturated solutions?
Why are supersaturated solutions of most solids in water prepared by cooling saturated solutions?
Given the observation that ethanol is completely miscible with water and ethanethiol is soluble only to the extent of 1.5 g per 100 mL of water, what can be inferred about their molecular structures?
Given the observation that ethanol is completely miscible with water and ethanethiol is soluble only to the extent of 1.5 g per 100 mL of water, what can be inferred about their molecular structures?
What would be the most likely reason for CH4 to be the most soluble gas in water among the given options?
What would be the most likely reason for CH4 to be the most soluble gas in water among the given options?
How did the concentration of dissolved CO2 in the beverage change when the bottle was opened?
How did the concentration of dissolved CO2 in the beverage change when the bottle was opened?
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