  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?

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...

Want to see the full answer?

See Solution

Want to see this answer and more?

Our solutions are written by experts, many with advanced degrees, and available 24/7

See Solution
Tagged in

Chemistry 