If O2 is collected over water at 40 ∘C and a total pressure of 742mmHg , what volume of gas will be collected?
I have this much info: P of O2 = 0.903 atm. T of H2O = 313K. Where do I take this from here?
Update:This is all the problem gives:
Consider the reaction: 2NiO(s)→2Ni(s) O2(g)
If O2 is collected over water at 40 ∘C and a total pressure of 742mmHg , what volume of gas will be collected for the complete reaction of 25.22g of NiO?
More Questions From This User See All
Answers & Comments
Verified answer
2 NiO → 2 Ni + O2
(25.22 g NiO) / (74.69287 g NiO/mol) x (1 mol O2 / 2 mol NiO) = 0.168825 mol O2
The source below says the vapor pressure of water at 40°C is 55.324 mmHg.
V = nRT / P = (0.168825 mol) x (62.36367 L mmHg/K mol) x (40 + 273 K) /
(742 mmHg - 55.324 mmHg) = 4.80 L
What is the mass or moles of O2 ?