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Compute the standard free enegry of the ...

Compute the standard free enegry of the reaction at `27^(@)C` for the combustion fo methane using the give data:
`CH_(4)(g) +2O_(2)(g) rarr CO_(2)(g) +2H_(2)O(l)`
`{:(Species,CH_(4),O_(2),CO_(2),2H_(2)O(l)),(Delta_(f)H^(Theta)(kJmol^(-1)),-74.8,-,-393.5,-285.8),(S^(Theta)(JK^(-1)mol^(-1)),186,205,214,70):}`

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Compute the standard free energy of the reaction at 27^(@)C for the combustion of methane using the given data. CH_(4)(g)+2O_(2)(g)to CO_(2)(g)+2H_(2)O(l) {:("Species",CH_(4),O_(2),CO_(2),H_(2)O),(Delta_(f)H^(@)//(kJ mol^(-1)),-74.8,-,-393.5,-285.8),(S^(@)//(JK^(-1)mol^(-1)),186,205,214,70):}

Compute the Gibbs energy change of the reaction at 27^(@)C for the combustion of methane. {:(" "CH_(4)(g)+2O_(2)(g)rarr CO_(2)(g)+2H_(2)O(l)),(Delta_(f)H^(Θ)("in kh mol"^(1))" "-74.8 " "- " "-393.5 " "-285.8),(S_(m)^(Θ)("in J K^(-1)mol"^(-1))" 186 205 214 70"):}

Compute the Gibbs energy change of the reaction at 27^(@)C for the combustion of methane. {:(" "CH_(4)(g)+2O_(2)(g)rarr CO_(2)(g)+2H_(2)O(l)),(Delta_(f)H^(Θ)("in kh mol"^(1))" "-74.8 " "- " "-393.5 " "-285.8),(S_(m)^(Θ)("in J K^(-1)mol"^(-1))" 186 205 214 70"):}

Compute the standard free energy of the reaction at 27^@C for the combustion of methane CH_4(g) + 2O_2(g) to CO_2(g) +2H_2O(l) using the following data : Also comment on the feasibility of the reaction.

Calculate the standard free energy change for the formation of methane at 300K : C("graphite") +2H_(2) (g) rarr CH_(4)(g) The following data are given: Delta_(f)H^(Theta) (kJ mol^(-1)): CH_(4)(g) =- 74.81 Delta_(f)S^(Theta)(JK^(-1) mol^(-1)): C("graphite") = 5.70, H_(2)(g) = 130.7 CH_(4)(g) = 186.3

Use the standard enthalpies of formation and calculation the enthalpy changes accompanying the following reaction: a. CH_(4)(g)+2O_(2)(g) rarr CO_(2)(g)+2H_(2)O(l) Given, enthalpies of formation of CH_(4) ,CO_(2) and H_(2)O are 74.8 kJmol^(-1) ,−393.5 kJmol^(−1) ,−286 kJmol^(−1) respectively.

Calculate the standard free energy change for the formation of methane at 300K : C("graphite") +2H_(2) (g) rarr CH_(4)(g) The following data are given: Delta_(f)H^(Theta) (kJ mol^(-1)): CH_(4)(g) =- 74.81 Delta_(f)S^(Theta)(JK^-1 mol^(-1)): C("graphite") = 5.70, H_(2)(g) = 130.7, CH_(4)(g) = 186.3

Calculate the enthalpy change for the reaction CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O(l) The enethalpy of formation of CH_(4)(g),CO_(2)(g) and H_(2)O(l) are -74.8 kJ mol^(-1) , -393.5 kJ mol^(-1) and -285.8 kJ mol^(-1) respectively.