Consider the reaction 3CH4(g)= C3H8(g)+ 2H2(g).Calculate Delta G at 298 K if the reaction mixture consists of 40 atm of CH4 , 0.011 atm of C3H8, and 2.1×10−2 atm of H2.
To calculate the standard Gibbs free energy change (ΔG°) for the reaction at 298 K, you need to use the equation:
ΔG° = ΔG°f (products) - ΔG°f (reactants)
where ΔG°f represents standard Gibbs free energy of formation.
First, we need to find the standard Gibbs free energy of formation for each compound involved in the reaction. These values are usually provided in a table or can be found in reference books.
The standard Gibbs free energy of formation for CH4 is 0 kJ/mol.
The standard Gibbs free energy of formation for C3H8 is -26.7 kJ/mol.
The standard Gibbs free energy of formation for H2 is 0 kJ/mol.
Now, we can calculate the standard Gibbs free energy change for the reaction:
ΔG° = [ΔG°f (C3H8) + 2ΔG°f (H2)] - 3ΔG°f (CH4)
= [-26.7 kJ/mol + 2(0 kJ/mol)] - 3(0 kJ/mol)
= -26.7 kJ/mol
So, the standard Gibbs free energy change (ΔG°) for the given reaction at 298 K is -26.7 kJ/mol.
Note that the given reaction equation and concentrations provided are not needed to calculate ΔG°. It only requires the standard Gibbs free energy of formation values for each compound involved in the reaction.