In
a Container 8g O2 , 7g Na
and 2g CH4 gases are present. What
is the total pressure of the mixture of the gas
at 25 centigreade .if the volume
of container is 11.2 dm3.
Answers
At STP conditions one mol of any gas has a volume of 22.4 litres.
STP conditions are 0 degrees Celsius and 1 atm pressure.
molar mass of O2 is 16 g, so 8 g is 0.5 mol.- 11.2 litres at stp.
molar mass of N2 is 14 g, so 7 g is 0.5 mol- 11.2 litres at stp.
molar mass of CH4 is 16 g, so 2 g is 0.125 mol- 2.8 litres at stp.
Hence, at stp the total volume of gases is 25.2 litres or 25.2 dm^3.
At STP: As mentioned in question:
V1=25.2 litres. V2=11.2 litres ( 1 dm3=1 litre)
P1= 1 atm P2=?
T1= 273 K T2=25 C=> 25 + 273 K=>298 K
By gas equation,
P1V1/T1=P2V2/T2=K(constant)
1 X 25.2/273=P2 X 11.2/298
P2=9.824 atm (approx.)
Hence the pressure will be about 9.82 atm.
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