Answer –Charles law states that the volume of a given mass of gas is directly proportional to its absolute temperature or temperature provided the pressure remains constant
(b) Draw a graphical representation of Charles Law
Answer –
(c) What is absolute zero temperature.
Answer – Absolute temperature is the temperature at which the molecules of a gas have no volume, no kinetic energy (no velocity), and no pressure.
State its value in
(i) Celsius temperature
Answer – -2730C
(ii) Kelvin temperature
Answer – 0K
Question 2
(a) A fixed mass of gas has a volume of 92cm3 at 30C. What will be its volume at 180C, if the pressure remains constant?
(b) Explain Charles Law in terms of Kinetic Theory
Answer – An increase in temperature gives rise to an increase in the average kinetic energy and the molecules of gas move more rapidly and collide with the walls of the container. At constant pressure, the volume of the container increase with an increase in temperature. Conversely, a decrease in temperature lowers the average kinetic energy of the gas molecules and also lowers the frequency of collision of gas molecules.
Question 3
(a) What volume would a gas occupy at s.t.p if at 430C and 720mmHg it occupies 214cm3
Answer – In a mixture of gases that do not react chemically together, the total pressure exerted by the mixture is equal to the sum of the partial pressures of the individual gases present in the mixture.
(b) 210cm3 of Nitrogen at a pressure of 400mmHg and 180cm3 of Carbon(IV) Oxide at a pressure of 350mmHg were introduced into a 200cm3 vessel. What is the total pressure in the vessel?
Answer –
N2
CO2
Vol ⇒ 210cm3
Vol ⇒ 180cm3
Pressure ⇒ 400mmHg
Pressure ⇒ 350mmHg
Volume of the vessel = 200cm3
:- \(\frac{Volume \; of \; the \;gas}{Volume \; of \; the \;vessel} \; \times \; \frac{Pressure \; of \;the\;gas}{1} \)
N2
CO2
\(\frac{210}{200} \; \times \; \scriptsize 400 \)
\(\frac{180}{200} \; \times \; \scriptsize 350 \)
= 420mmHg
= 315mmHg
According to Dalton’s law of partial pressure,
Ptotal = Pa + Pb + Pc … + Pn
Ptotal = PN2 + PCO2
Ptotal = 735mmHg
Question 5
Two vessels contain separately 50cm3 of Nitrogen at 100mmHg pressure and 80cm3 of Oxygen at 200mmHg and they are connected by taps to a third vessel containing 30cm3 of Hydrogen at 500mmHg. If the taps are opened and the gases are allowed to mix until equilibrium is attained, determine
(a) The partial pressure of each of the three gases
Answer – Total volume of the gases (N2 + O2 + H2) = 50 + 80 + 30 = 160cm3
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