Answer:

A perfect gas at 27°C is heated at constant pressure till its VOLUME is doubled. What will be its final temperature?

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Using gas equation, we have

(P1*V1) /T1=(P2*V2) /T2 where P=Pressure, V=Volume and T=Absolute temperature of the gas.

Given, P1=P2=P(say) (Since pressure is constant)

V1=V(say), where V is the initial volume of the gas.

Therefore, V2=2V since final volume is double the initial volume.

T1=(27+273)K=300K

T2=?

Substituting the values obtained,in the gas equation, we have

P*V/300=P*2V/T2

Solving, we get T2=final temperature of the gas=600K or (600–273)degree C or 327 degrees C.

Explanation:

Ideal gas equation is pv= mRT ,

In present case , pressure is constant. Thus ideal gas equation can be rewritten as

v/T = mR/p = constant ( since 'mass' and 'characteristic gas constant' are going to be remain same)

Thus,

T2/T1 = v2/v1 ( but in question it was given, v2 = 2×v1)

That is,

T2/(27+273) = 2× v1/v1 ( 273 is added with 27°C to convert in Kelvin)

T2=2×300

T2= 600 k i.e. 327°C( that is your final temperature)