I have a sealed container that is pressurised with Nitrogen- When calc.docx
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The document discusses the calculation of gas density in a pressurized container filled with nitrogen. It clarifies that the molar mass to use is that of N2 (28.0134 g/mol) instead of nitrogen atoms (14.0067 g/mol) because the pressure comes from the N2 gas, not from individual nitrogen atoms. The discussion references the ideal gas equation to support this conclusion.
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I have a sealed container that is pressurised with Nitrogen- When calc.docx
- 1. I have a sealed container that is pressurised with Nitrogen. When calculating the density of a gas inside a container using d = (M * P) / (R *T) M = molar mass, P = pressure, R = gas constant, T = temperature. When putting in the molar mass for nitrogen do i need to put in the value of N = 14.0067, or that of N2 = 28.0134, given that N2 is the natural state? Also, why? Thank you Solution See, the pressure in the container is due to N2 gas not due to N atoms. So, the molar mass that should be taken is of N2 gas. Also, this expression is basically derived from ideal gas equation: PV = n RT Where n is number of moles of gas n = given mass of gas(m)/molar mass of gas(M) Here molar mass is for gas( if nitrogen then N2) PV = mRT/M PM = mRT/V P×M/(R×T) = m/ V = d d = P*M/(R*T) So, molar mass taken is of N2