Home
Class 12
CHEMISTRY
Compute the standard free energy of the ...

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):}`

Text Solution

AI Generated Solution

To compute the standard free energy change (ΔG°) for the combustion of methane at 27°C, we will follow these steps: ### Step 1: Write the Reaction The balanced chemical reaction for the combustion of methane is: \[ \text{CH}_4(g) + 2\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\text{H}_2\text{O}(l) \] ### Step 2: Gather Data From the provided data, we have: ...
Promotional Banner

Similar Questions

Explore conceptually related problems

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):}

Estimate the enthalpy of combustion of methane in KJ .mol^(-1) CH_(4)(g)+2O_(2)(g)to CO_(2)(g)+2H_(2)O(g)

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"):}

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.

The enthalpy of vaporisation of liquid water using the data H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l) , DeltaH=-285.77 kJ//mol H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(g) , DeltaH=-241.84 kJ//mol

Calculate the enthalpy of formation of methane from the following data : C(s) + O_(2)(g) to CO_(2)(g) Delta_(r)H^(@) = -393.5 kJ 2H_(2)(g) + O_(2)(g) to 2H_(2)O(l) Delta_(r)H^(@) = -571.8 kJ CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O(l) Delta_(r)H^(@) = -890.3 kJ

Calculate the standard Gibbs enegry change for the combustion of alpha-D glucose at 300K . C_(6)H_(12)O_(6)(s) +6O_(2)(g) rarr 6CO_(2)(g) +6H_(2)O(l) Given the standard enthalpies of formation (kJ mol^(-1)) C_(6)H_(12)O_(6) =- 1274.5, CO_(2) =- 393.5, H_(2)O =- 285.8 . Entropies (J K mol^(-1)) C_(6)H_(12)O_(6) = 212.1, O_(1) = 205.0, CO_(2) =213, H_(2)O = 69.9