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

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :

the answer is minerals.