Math

Question20. Gaseous O2\mathrm{O}_{2} in equilibrium with O2\mathrm{O}_{2} dissolved in water at 283 K is depicted at the right. (a: 1 Mark) Which scene or scenes below (A, B or C) represents the system at 298 K ? \qquad (b: 1 Mark) Which scene or scenes below (A, B or C) represents the system when the pressure of O2\mathrm{O}_{2} has been increased by half?

Studdy Solution

STEP 1

1. The system is initially at equilibrium at 283 K with equal numbers of O₂ molecules in the gaseous and dissolved states.
2. Increasing the temperature generally decreases the solubility of gases in liquids.
3. Increasing the pressure of a gas above a liquid generally increases the solubility of the gas in the liquid.

STEP 2

1. Analyze the effect of temperature increase on the system.
2. Analyze the effect of pressure increase on the system.
3. Match the scenes to the described conditions.

STEP 3

At 283 K, the system is in equilibrium with three O₂ molecules in the gaseous state and three in the dissolved state.
Increasing the temperature to 298 K typically decreases the solubility of gases in liquids, meaning more O₂ molecules should be in the gaseous state than in the dissolved state.

STEP 4

Increasing the pressure of O₂ by half should increase the number of O₂ molecules in the dissolved state compared to the gaseous state, as higher pressure increases solubility.

STEP 5

(a) For the system at 298 K, we expect more O₂ molecules in the gaseous state than in the dissolved state. Scene B, which shows six O₂ molecules in the gaseous state and three in the dissolved state, matches this condition.
(b) For the system with increased pressure, we expect more O₂ molecules in the dissolved state than in the gaseous state. Scene A, which shows two O₂ molecules in the gaseous state and five in the dissolved state, matches this condition.
The scenes that represent the system under the given conditions are:
(a) Scene B for the system at 298 K. (b) Scene A for the system with increased pressure.

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