Advertisements
Advertisements
Question
State Charles's law.
Advertisements
Solution
Charles's Law
At constant pressure, the volume of a given mass of a dry gas increases or decreases by 1/273rd of its original volume at 0°C for each degree centigrade rise or fall in temperature.
V ∝ T (at constant pressure)
At temperature T1 (K) and volume V1 (cm3):
`"V"_1 ∝ "T"_1 "or" "V"_1/"T"_1 = "K"` = constant...(i)
At temperature T2 (K) and volume V2 (cm3):
`"V"_2 ∝ "T"_2 "or" "V"_2/"T"_2 = "K"` = constant….(ii)
From (i) and (ii),
`"V"_1/"T"_1 = "V"_2/"T"_2` = constant
For Temperature = Conversion from Celsius to Kelvin
1 K = °C + 273
Example:
20°C = 20 + 273 = 293 K
APPEARS IN
RELATED QUESTIONS
Give the assumptions of the kinetic molecular theory.
Explain Charles's law on the basis of the kinetic theory of matter.
State the law which is represented by the following graph:
State the following:
Ice point in absolute temperature
88 cm3 of nitrogen is at a pressure of 770 mm mercury. If the pressure is raised to 880 mmHg, find by how much the volume will diminish, the temperature remaining constant.
Taking the volume of hydrogen as calculated in Q.19, what change must be made in Kelvin (absolute) temperature to return the volume to 2500 cm3 (pressure remaining constant)?
A certain mass of gas occupied 850 ml at a pressure of 760 mm of Hg. On increasing the pressure it was found that the volume of the gas was 75% of its initial value. Assuming constant temperature, find the final pressure of the gas?
It is required to reduce the volume of a gas by 20% by compressing it at a constant pressure. To do so, the gas has to be cooled. If the gas attains a final temperature of 157°C, find the initial temperature of the gas.
A fixed volume of a gas occupies 760cm3 at 27°C and 70 cm of Hg. What will be its vol. at s.t.p.
The following question refers to one mole of chlorine gas.
What volume will it occupy at 273°C?
