Determine Delta S degree for the following reaction: CH_4(g) + 2O_2,(g) CO_2(g)+

Question

Determine Delta S degree for the following reaction: CH_4(g) + 2O_2,(g) CO_2(g)+2H2,O(l) Consider the following hypothetical reaction, at T - 310.4K. Standard free energies, in kJ/mol. arc given in parentheses. (Then Delta G degree - 7) A rightarrow B + C (-29.8) (-207.8) (+237.0) What is the value of the equilibrium constant K for this reaction, at this temperature? Draw a sketch of the electrochemical cell: Ag(s) | Ag^+ (aq) || Cd^2+'(aq) | Cd(s) Include and label the anode, cathode, wire with direction of flow of electrons, voltmeter (no volage value), salt bridge, and cach solid metal and metal ion in the appropriate place.

Explanation / Answer

CH4+2O2-----> 2H2O +CO2

Delta S = delt S products - Delta S reactants

                = 2*69.95 +213.7-(186.1+2*205)

                 = 139.9 +213.7 - 596.1

               = -242.5j/mole-k

A---------------> B+C

Delt G = Delta G products - DElta G reactants

          = -207.8+237 -(-29.8)

         = 59Kj/mole

Delta G = -RTlnK

59000 = -8.314*310*2.303logK

59000 = -5935.614logK

logK = - 59000/5935.614   = -9.939

K     = 10-9.939       = 1.15*10-10

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