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Sabra_a

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- Homework Statement
- Three 60-litre high-pressure gas cylinders contain gaseous fire suppressants. The suppressants are:

1) IG-100 (which is 100% N2),

2) Carbon dioxide (CO2),

3) IG-55 (50% vol. N2 and 50% vol. Ar).

The suppressants are stored in gaseous form under the pressure 170 atm (1 atm=101325 Pa) and at normal temperature (T=293K).

(i) Calculate the mass fraction of nitrogen and argon in gas mixture IG-55.

(ii) Assume ideal gas behaviour of the suppressants. What is the mass of the gas contained in each cylinder?

(iii) The suppressants are to be released in an environment at normal conditions of pressure and temperature (p=1atm, T=293K). What volume will be occupied by each suppressant after their release into the environment? Assume isothermal expansion in your calculation.

Note: atomic masses: M(N)=14 kg/kmol, M(Ar)=40 kg/kmol, M(C)

=12 kg/kmol, M(O)=16 kg/kmol.

- Relevant Equations
- mass fraction

atomic mass

molecular mass

ideal gas equation

I have attached the full answer in PDF file. I'm not sure about the answers. will really appreciate if they get checked