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A 2.0 L container at 25^(@)C contain 1.2...

A 2.0 L container at `25^(@)C` contain 1.25 mol of `O_(2)` and 3.2 mol of C.
(a) What is the initial pressure in the flask ?
(b) If the carbon and oxygen react as completely as possible to form `CO,` what will be the final pressure in the container?

Text Solution

Verified by Experts

The container contains 1.25 mol of `O_(2)` and 3.2 mol of C. Since only oxygen is gaseous and carbon will not exert any pressure.
`n=1.25 mol, V = 2.0L, T=273+25=298K`
`therefore" "p=(nRT)/(V)`
`=(("1.25 mol")xx("0.0821 L atm mol"^(-1)"K"^(-1))("298 K"))/(("2.0 L"))`
`="15.3 atm"`
(b) The reaction is
`C+(1)/(2)O_(2)rarrCO`
According to the equation, 1 mol of `CO` will be produced for every `(1)/(2)` mol of `O_(2)` used.
`(1)/(2)" mole of "O_(2)" gives CO = 1 mole"`
`"!.25 mole of "O_(2)" will give CO"=1xx2xx1.25`
`="2.50 mol"`
The final pressure is
`p=(("2.50 mol")xx("0.0821 L atm"^(-1)"K"^(-1)"mol"^(-1))xx("298 K"))/(2.0L)`
`=30.6atm.`
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