Having trouble trying to solve this chem homework question. Its pretty difficult to solve.
If all the H20(g) in the atmosphere (assume it is 1% by volume) suddenly condensed to H20(l), and all the enthaply of this process was captured and converted to electrical energy, how long would this energy power an average size city of 1 million?
I know that atmospheric water vapor volume is 12.9 cubic kilometers, but cant figure out the rest.
2006-11-24 03:40:48 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
24 litres of air (at RTP) will contain 1 mole of gas. You are told that you have 12.9 cubic kilometres of water vapour. Convert this to litres, and then to moles The enthalpy of vaporisation of water is 40.65kJ/mol, so you can now work out the total energy released.
You would also need to research the power consumption of a city of 1 million people!
2006-11-25 21:36:22 · answer #1 · answered by Gervald F 7 · 0⤊ 0⤋
an consumer-friendly thank you to ingredient a trinomial into 2 binomials is via making the main applicable coefficient one million. 28) 2(t^2 + 4t - 32) = 0 ingredient t^2 + 4t - 32: 2(t + 8)(t - 4) = 0 29) 3(a^2 - 12a + 27) 3(a - 9)(a - 3) = 0 you ought to be conscious of the place to flow from those spots. desire I helped!
2016-12-17 15:33:09 · answer #2 · answered by Anonymous · 0⤊ 0⤋