Question

In a container 8g O2, 7g N2 and 2g CH4 gases are present.what is the total pressure of the mixture of the gas at 25°C if the volume of the container is 11.2dm3

Answer 1

Answer:

Chemistry

5 points

ANSWER

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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