Question

. If 50 mL of oxygen gas at 27°C is heated to 45°C,
under constant pressure then final volume of the
gas will be
X (1) 57 mL
(2) 53 mL
(4) 60 mL
(3) 62 mL​

Answer 1

Explanation:

use Charles law

v1/v2=t1/t2

50/v=300/318

solve this u get urs answer perfectly

Answer 2

Answer:(2) 53ml

Explanation:

Given:-

50ml of oxygen gas at initial temperature of 27C:-

V(initial)=50ml

T(initial)=27C(Need to convert temperature into Kelvin):-

Temperature in K is equal to Temperature in C +273.

Initial Temperature in K is 27+273=300K

It is heated to 45C at constant pressure.

Final Temperature in K is 273+45=318K.

This follows the conditions that at constant pressure temperature is proportional to Volume by Charle's law as:-

This is because in the Ideal Gas Law:-PV=nRT,

We have P=constant, n,R=Constant so,

It is given in the question that pressure is constant,

Now n(Moles in the container remain constant)

And finally The value of R only depends on units but is an universal constant:-

R=0.0821atmL/mole-K

R=8.314J/K or R=2cal/K.

Now this equation we have two equations:- For final and initial states:-

PfVf=nRTf-----(1)

PiVi=nRTi-----(2)

And divide these equations to give the charles law.

Volume is directly proportional to Temperature(in K)

So,

Vf/Vi=Tf/Ti;

Vf/50ml=318K/300K,

So,

Vf=(318×50)/300 in ml,

Vf=318/6 in ml = 53ml(Answer).

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