Advertisements
Advertisements
Question
Explain the following observation.
Aerated water bottles are kept under water during summer
Advertisements
Solution
In aerated water bottles, CO2 gas is passed through the aqueous solution under pressure because the solubility of the gas in water is not very high. In summer, the solubility of the gas in water is likely to decrease because of the rise in temperature. Thus, in summer, more gas will be present above the liquid surface in the glass bottle.
In case, the pressure of the gas becomes too high, the glass will not be able to withstand the pressure and the bottle may explode. To avoid this, the bottles are kept under water. As a result, the temperature is likely to decrease and the solubility of CO2 is likely to increase in aqueous solution resulting in decreased pressure.
APPEARS IN
RELATED QUESTIONS
State the following:
The absolute temperature of a gas at 7°C
Convert the following temperature from degree Celcius to kelvin.
−15° C
Convert the following temperature from degree Celcius to kelvin.
25° C
Convert −100° C to kelvin
Consider a sample of a gas in a cylinder with a movable piston.
Show diagrammatically the changes in the position of the piston, if pressure is increased from 1.0 bar to 2.0 bar at a constant temperature.
Match the pairs of the following:
| Column ‘A’ | Column ‘B’ |
| a. Boyle’s law | i. at constant pressure and volume |
| b. Charles’ law | ii. at constant temperature |
| iii. at constant pressure |
Write the statement for Boyle’s law
With the help of the graph answer the following -
At constant temperature, Write the statement of law.
Solve the following.
The volume of a given mass of a gas at 0°C is 2 dm3. Calculate the new volume of the gas at constant pressure when the temperature is decreased by 10°C.
Name two items that can serve as a model for Gay Lusaac’s law and explain.
