Advertisements
Advertisements
प्रश्न
Solve the following.
A balloon is inflated with helium gas at room temperature of 25°C and at 1 bar pressure when its initial volume is 2.27L and allowed to rise in the air. As it rises in the air external pressure decreases and the volume of the gas increases till finally, it bursts when external pressure is 0.3bar. What is the limit at which the volume of the balloon can stay inflated?
Advertisements
उत्तर
Given:
P1 = Initial pressure = 1 bar
V1 = Initial volume = 2.27 L
P2 = Final pressure = 0.3 bar
To find: V2 = Final volume
Formula: P1V1 = P2V2 (at constant n and T)
Calculation:
According to Boyle’s law,
P1V1 = P2V2 (at constant n and T)
∴ V2 = `("P"_1"V"_1)/"P"_2=(1xx2.27)/0.3` = 7.566667 L ≈ 7.567 L
The balloon can stay inflated below the volume of 7.567 L.
APPEARS IN
संबंधित प्रश्न
Explain Why?
"When stating the volume of a gas, the pressure and temperature should also be given."
What would be the mass of CO2 occupying a volume of 44 litres at 25°C and 750 mm pressure.
Give reason for the following:
Gases have a lower density compared to solids or liquids.
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.
273° C
Convert the following pressure value into Pascals.
10 atmosphere
Convert the following pressure value into Pascals.
107000 Nm−2
Convert exactly 1.5 atm to pascals
Identify the gas laws from the following diagram.
| Diagram | Gas laws |
 |
______________ |
Identify the gas laws from the following diagram.
| Diagram | Gas laws |
 |
______________ |
Write the statement for Charles’ law
With the help of the graph answer the following -
At constant temperature, the Graph shows the relationship between pressure and volume. Represent the relation mathematically.
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 increased by 10°C.
Solve the following.
At 0°C, a gas occupies 22.4 liters. How much hot must be the gas in celsius and in kelvin to reach a volume of 25.0 liters?
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
Give the mathematical expression that relates gas volume and moles.
Of two samples of nitrogen gas, sample A contains 1.5 moles of nitrogen in a vessel of the volume of 37.6 dm3 at 298 K, and sample B is in a vessel of volume 16.5 dm3 at 298 K. Calculate the number of moles in sample B.
For a given mass of an ideal gas, which of the following statements is CORRECT?
A certain sample of gas has a volume of 0.2 L at one atmosphere pressure and 273.15 K. What is the volume of gas at 273.15°C at same pressure?
At what temperature the volume of a gas becomes absolutely zero?
Isochor is the graph plotted between ______.
The volume of 400 cm3 chlorine gas at 400 mm of Hg is decreased to 200 cm3 at constant temperature. What is the new pressure of gas?
10 g of gas at one atomospheric pressure is cooled from 273.15°C to 0°C keeping the volume constant. What is the final pressure?
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.
