You have to convert 20° C to Kelvin; you can't just plug it into the equation
PV=nRT
P=nRT/V=[(0.65moles)(0.082)(293.15K)]/4.0L
P=3.9 atm
A 0.65 mole quantity of O2 occupies 4.0 L at 20.◦C. What is the final pressure exerted by the gas?
1. 0.92 atm
2. 3.9 atm
3. 6.2 atm
4. 1.1 atm
5. 0.27 atm
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Initially, I got .27 atm. I got this answer by plugging in the values into the equation [pv=nRT], coming out as [p*4=0.65*.082*20]. However, my assignment says this answer is wrong. May someone explain to me my error? Am I overlooking something? Thank you in advance~
4 answers
All data dimensions must match the units of the Universal Gas Constant (R) being used... For your problem R = 0.08206 L-Atm/mole-K.
I see. Thank you!
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