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CH4(g) + 2O2(g) CO2(g) + 2H2O(l)This  reaction occurs spontaneously as written when all reactants and products are in their standard states. T = 298.17 K)What is G° for this reaction in J/mol?

Question

CH4(g) + 2O2(g) CO2(g) + 2H2O(l)

This  reaction occurs spontaneously as written when all reactants and products are in their standard states. T = 298.17 K)

What is G° for this reaction in J/mol?

check_circleAnswer
Step 1

Step 1:

 

The standard Gibbs energy change for a process is defined as a change in which the reactants in the standard states are converted to products in their standard state.

 

The standard Gibbs energy change of a reaction is calculated with the help of equation written below:

∆G =⅀∆fG(products)- ⅀∆fG(reactants)

Step 2

Step 2:

 

The given reaction is,

CH4(g)+2O2 → CO2(g)+2H2O(l)

 

The standard values are,

 ∆fG [CO2(g)] = -394.4 kJmol-1

fG[ H2O(l)] = -237.2 kJmol-1

fG [CH4(g)] = -50.8 kJmol-1

fG[O2(g)] =0 kJmol-1

 

 

The ∆G for the above reaction is calculated as follows:

∆G={∆fG [CO2(g)] + 2∆fG[ H2O(l)]} -{∆fG [CH4(g)] + 2∆fG[O2(g)]}

 

Substitute the standard values in the above equation as,

∆G ={(-394.4 kJmol-1 )+ (2×-237.2 kJmol-1} -{(-50.8 kJmol-1)+ (2×0 kJmol-1)}

∆G=-818 kJmol-1

Step 3

Step 3:

 

The relation between kJmol-1 and Jmol-1 is written below:

 

1 kJmol-1 = 1000 Jmol-1

Now, convert -818 kJmol-1 by using the ab...

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