Methane, a component in natural gas, can be used as a fuel in combustion reactions. what is the value for δgnon (in kj) for the following reaction under the given conditions at 293 k? ch4 (g) + 2 o2 (g) → co2 (g) + 2 h2o (g) where δhorxn = -803 kj, δsorxn = -4.05 j/k, and [ch4] = 14.51 m, [o2] = 9.27 m, [co2] = 3.83 m, and [h2o] = 6.41 m. (in kj)

The for the reaction is -806.86 kJ

Explanation:

We are given:

     (Conversion factor:  1 kJ = 1000)

Temperature of the reaction = 293 K

To calculate the standard Gibbs's free energy of the reaction, we use the equation:

Putting values in above equation, we get:

For the given chemical equation:

The expression for is given as:

We are given:

Putting values in above equation, we get:

To calculate the Gibbs free energy of the reaction, we use the equation:

where,

= Gibbs' free energy of the reaction = ?

= Standard gibbs' free energy change of the reaction = -801813.35 J

R = Gas constant =

T = Temperature = 293 K

= equilibrium constant in terms of concentration = 0.126

Putting values in above equation, we get:

Hence, the for the reaction is -806.86 kJ

it is a good conductor

explanation: