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Using the ideal gas law, calculate the density of CO2 at 4.00 atm pressure and -20.0 oC.
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- P = 4.00 atm
- T = -20.0 + 273.15 = 253.15K
- R = 0.08206 atm-L/mol-K
- Molar mass of CO_2 = 44.01 grams/mol
Using the Ideal gas law we can solve for the density of gas. First, let us write down the Ideal gas equation and the formula for density.
`PV = nRT`
`rho = (mass)/(volume) = M/V`
We know that moles = mass (M)/ molar mass, so we can substitute it to the Ideal gas equation thus having:
`PV = (M)/(molar mass) * RT`
Further arrangement in the expression we can have:
`(P)/(RT) =(M)/(molar mass * V)`
`(P* molar mass)/(RT) =(M)/(V)= rho`
`rho =(P* molar mass)/(RT)`
`rho =(4.00* 44.01)/(0.08206* 253.15)`
`rho` = 8.47 g/L = 0.00847 g/ml
Posted by jerichorayel on April 8, 2013 at 6:11 AM (Answer #1)
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