1) What is Boyle's temperature
2)(a) Define (i) critical temperature (ii) critical pressure (iii) critical volume
3) What will be the minimum pressure required to compress 500 dm air at I bar pressure to 200 dm³ at 30 degree Celsius?
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Answers
Answer:
Explanation:
1. Temperature at which real gas obeys the gas laws over a wide range of pressure is called Boyle's Temperature.
2. i) The temperature of a gas in its critical state, above which it cannot be liquefied by pressure alone.
ii) The pressure of a gas or vapour in its critical state.
iii) The volume occupied by a unit mass of a gas or vapour in its critical state.
3. P₁ = 1
P₂ = ?
V₁= 500 dm³
V₂= 200 dm³
Apply boyle's law p₁V₁=p₂V₂ to calculate p₂ as temperature remains constant.
p₂ = p₁V₁/ V₂ = 1 bar × 500 dm³/ 200 dm³ = 2.5 bar
2.5 is the required answer !
Answer:
1) At constant temperature pressure of a given mass of gass is inversely proportional to volume
P1V1=P2V2
2) (i) It is the maximum temperature in which a gas can be liquified by the application of pressure
(ii) It is volume occupied by 1 mole of a gas at critical temperature and critical pressure
3) V1=500 dm3
P1=1 bar
V2=200dm3
T1= 30+273K =303K
P2=?
P1V1=P2V2
P2=P1V1/V2
P2= 1x500/200
P2=2.5 bar
Explanation: