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
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.
State the following:
The absolute temperature of a gas at 7°C
Answer in one sentence.
A bubble of methane gas rises from the bottom of the North sea. What will happen to the size of the bubble as it rises to the surface?
Convert the following temperature from degree Celcius to kelvin.
−15° C
Convert the following temperature from degree Celcius to kelvin.
−197° C
Convert the following pressure value into Pascals.
107000 Nm−2
Convert 0.124 torr to the standard atmosphere
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.
The temperatures at which real gases obey the ideal gas laws over a wide range of pressure is called __________.
State Boyle's law.
Explain the following observation.
Liquid ammonia bottle is cooled before opening the seal
A sample of gas at 15°C at 1 atm. has a volume of 2.58 dm3. When the temperature is raised to 38°C at 1 atm does the volume of the gas Increase? If so, calculate the final volume.
Hydrochloric acid is treated with a metal to produce hydrogen gas. Suppose a student carries out this reaction and collects a volume of 154.4 × 10−3 dm3 of a gas at a pressure of 742 mm of Hg at a temperature of 298 K. What mass of hydrogen gas (in mg) did the student collect?
At 25°C and 1 atm, a cylinder containing 10 L of an ideal gas is connected to the empty cylinder with a capacity of 20 L. The pressures exerted by gas m both the cylinders will be ____________.
For a given mass of an ideal gas, which of the following statements is CORRECT?
According to Andrews isothermals, the minimum temperature at which carbon dioxide gas obeys Boyles law is ______.
At what temperature the volume of a gas becomes absolutely zero?
Isochor is the graph plotted between ______.
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?
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?
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)
At what temperature, the volume of gas would become zero?
Identify the correct relationship between pressure (P), density (d), molar mass (M) and Temperature (T) for an ideal gas from the following.
