Question

4. (11.11) The combustion of hydrogen is a reaction that is known to "go to completion." a. Use data in Appendix H to evaluate the thermodynamic equilibrium constant at 298.15 K for the reaction H2(g) + {O2(g) → H2O(1) b. Assume that the reaction is at equilibrium at 298.15 K in a system in which the partial pressure of O2 is 1.0 bar. Assume ideal-gas behavior and find the equilibrium partial pressure of Hz and the number of H2 molecules in 1.0 m of the gas phase.

I wasn't given the partial pressures so why do you need it? can the problem really not be solved without it?

1 bar for each

Answer 1

Reactesn takig foe a) AG AG A DG from the Values aivan in table AGO -237.13 -0+0 KJIMOL www AG0-237.13 KJMOL AG=-RTAnK La ko= -AGO RT

nko= 237.13 xlo n5.67 Xo mol C314 298.15 1 md el Costaurs 6.022xlonoleules ll0.1855 5.67 xl44 raal K = 7128 x10 Equilibrium Constant 6.022x23 x5.6tx1 froleaks 1 ( t )H No- of moleule = 3.414xlo23 mokuk at hs fastal be and nukes e mdewles H at eam rere Laleubte Liquids ond selids tae do not Qrest fartial Aren nd tter Valuas ase not taken iot LThe heactin almast GOES TO CatMPLETIDN Consideaation 1 PH(2 1 ko.(1 7.128 xl PH=1.403x1o equiliboun Poeur ef 46 bar PV=nRT P n=PV= 403x1dax Im RT 0.083 Lbramol x 24-5 1-48 5.67 xb0 L Moc (: 11-16m) n= 5.67x1050m mott