Advertisements
Advertisements
Question
Hot air balloons float in the air because of the low density of the air inside the balloon. Explain this with the help of an appropriate gas law.

Advertisements
Solution
The working of a hot air balloon can be explained with the help of Charles’ law. According to Charles’ law, at constant pressure, the volume of a fixed amount of a gas varies directly with the temperature. This means that as the temperature increases, the air inside the balloon expands and occupies more volume. Thus, hot air inside the balloon is less dense than the surrounding cold air. This causes the hot air balloon to float in the air.
APPEARS IN
RELATED QUESTIONS
State (i) the three variables for gas laws and (ii) SI units of these variables.
Give reason for the following:
Gases exert pressure in all directions.
Convert the following temperature from degree Celcius to kelvin.
−15° C
Convert the following temperature from degree Celcius to kelvin.
25° C
Convert the following temperature from degree Celcius to kelvin.
−197° C
Convert the following temperature from degree Celcius to kelvin.
273° C
Convert the following pressure value into Pascals.
1 kPa
Identify the gas laws from the following diagram.
| Diagram | Gas laws |
![]() |
______________ |
Identify the gas laws from the following diagram.
| Diagram | Gas laws |
![]() |
______________ |
Consider a sample of a gas in a cylinder with a movable piston.

Show diagrammatically the changes in the position of the piston, if the temperature is decreased from 300 K to 150 K at constant pressure.
Consider a sample of a gas in a cylinder with a movable piston.

Show diagrammatically the changes in the position of the piston, if the temperature is decreased from 400 K to 300 K, and pressure is decreased from 4 bar to 3 bar.
Assertion: Critical temperature of CO2 is 304 K, it can be liquefied above 304 K.
Reason: For a given mass of gas, volume is to directly proportional to pressure at constant temperature
Name two items that can serve as a model for Gay Lusaac’s law and explain.
Give the mathematical expression that relates gas volume and moles.
Explain the following observation.
Aerated water bottles are kept under water during summer
Explain the following observation.
Liquid ammonia bottle is cooled before opening the seal
Explain the following observation.
The type of an automobile is inflated to slightly lesser pressure in summer than in winter
Sulphur hexafluoride is a colourless, odourless gas; calculate the pressure exerted by 1.82 moles of the gas in a steel vessel of volume 5.43 dm3 at 69.5 °C, assuming ideal gas behaviour
According to Andrews isothermals, the minimum temperature at which carbon dioxide gas obeys Boyles law is ______.
Volume of a balloon at 25°C and 1 bar pressure is 2.27 L. If the pressure of the gas in balloon is reduced to 0.227 bar, what is the rise in volume of a gas?
A certain mass of a gas occupies a volume of 2 dm3 at STP. At what temperature the volume of gas becomes double, keeping the pressure constant?
At what temperature the volume of a gas becomes absolutely zero?
A gas occupies a volume of 4.2 dm3 at 101 kPa pressure. What volume will gas occupy if the pressure is increased to 235 kPa keeping the temperature constant?
If 2 moles of an ideal gas at 546 K has volume of 44.8 L, then what will be it's pressure? (R = 0.082)
If 300 mL of a gas at 26.85°C is cooled to 6.85°C at constant pressure. What will be the final volume of gas?
At what temperature, the volume of gas would become zero?
The number of molecules in 8.96 litres of gas at 0°C and 1 atm. pressure is approximately ______.
Identify the correct relationship between pressure (P), density (d), molar mass (M) and Temperature (T) for an ideal gas from the following.


