English

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

Advertisements
Advertisements

Question

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.

Diagram

Solution

At constant P, V ∝ T

Since the temperature becomes half, the volume will also become half.

shaalaa.com
The Gas Laws
  Is there an error in this question or solution?
Chapter 10: States of Matter - Exercises [Page 158]

APPEARS IN

Balbharati Chemistry [English] 11 Standard
Chapter 10 States of Matter
Exercises | Q 3. (B)(b) | Page 158

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 have a lower density compared to solids or liquids.


State the following:

The absolute temperature of a gas at 7°C


Convert the following temperature from degree Celcius to kelvin.

25° C


Convert the following temperature from degree Celcius to kelvin.

273° C


Convert the following pressure value into Pascals.

1 kPa


Convert the following pressure value into Pascals.

1 atmosphere


Convert exactly 1.5 atm to pascals


Convert 89 kPa to newton per square metre (Nm−2)


Convert 101.325 kPa to bar.


Convert 0.124 torr to the standard atmosphere


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
______________

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

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.

A hot air balloon has a volume of 2800 m3 at 99°C. What is the volume if the air cools to 80°C?


Use of hot air balloon in sports and meteorological observation is an application of


Name two items that can serve as a model for Gay Lusaac’s law and explain.


Explain the following observation.

Aerated water bottles are kept under water during summer


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.


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?


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


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 ____________.


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?


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×