Question

A sample of hydrogen gas occupies a volume of 300 ml
at 1.2 bar pressure and 50 C. Calculate its volume at 0.45 bar pressure and 700 C

Answer 1

Answer:

PV=nRT

If half of the mass of hydrogen occupy at triple the absolute temperature if the pressure were one-ninth the original gas,

Here initial no. of moles is half of the final no. of moles because molar mass is same both the time.

V

1

=

P

1

n

1

RT

1

=30 ml ----- 1

Again,

P

2

V

2

=n

2

RT

2

So

9

p

1

×V=

2

n

1

×R×3T

1

---- 2

From 1 and 2 equation

V=

2

9×30×3

=405 mL

Answer 2

Explanation:

Dear Student,

We know that, PV= nRTSo, n=PVRTn will be constant So, P1V1RT1=P2V2RT2or, P1V1T1=P2V2T2P1= 1.2 bar= 1.2 atmV1=300 ml = 0.3 LT1= 50°C= 50+273=323 KP2=0.45 bar=0.45 atmT2= 700°C= 700+273=973 KSo, V2=P1V1T2T1P2=1.2×0.3×973323×0.45=2.40 L