Advertisements
Advertisements
Question
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 |
Advertisements
Solution
| Column ‘A’ | Column ‘B’ |
| a. Boyle’s law | ii. at constant temperature |
| b. Charles’ law | iii. at constant pressure |
APPEARS IN
RELATED QUESTIONS
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 exert pressure in all directions.
Convert the following temperature from degree Celcius to kelvin.
−15° C
Convert the following pressure value into Pascals.
1 kPa
Convert the following pressure value into Pascals.
107000 Nm−2
Convert 89 kPa to newton per square metre (Nm−2)
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.
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, Write the statement of law.
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?
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.
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.
State Boyle's law.
Explain the following observation.
Aerated water bottles are kept under water during summer
Explain the following observation.
The size of a weather balloon becomes larger and larger as it ascends up to larger altitude
A sample of gas has a volume of 8.5 dm3 at an unknown temperature. When the sample is submerged in ice water at 0°C, its volume gets reduced to 6.37 dm3. What is its initial temperature?
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.
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 ____________.
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?
According to Andrews isothermals at what temperature the carbon dioxide gas starts to condense at 73 atmosphere?
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?
Isochor is the graph plotted between ______.
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)
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?
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?
