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°) at a given temperature for a reaction, you need to use the formula:

ΔG° = ΔG°f (products) - ΔG°f (reactants)

where ΔG°f is the standard Gibbs free energy of formation.

To calculate ΔG° for each compound, you can use the standard Gibbs free energy of formation values (ΔG°f) for each compound, which you can find in reference tables.

For the reaction you provided:

3CH4(g) = C3H8(g) + 2H2(g)

Let's assume the standard Gibbs free energy of formation for CH4, C3H8, and H2 are ΔG°f(CH4), ΔG°f(C3H8), and ΔG°f(H2), respectively.

The equation for ΔG° is:

ΔG° = [ΔG°f(C3H8) + 2ΔG°f(H2)] - [3ΔG°f(CH4)]

To calculate ΔG°, you need to find the values of ΔG°f for each compound at 298 K.

Once you have the values, substitute them into the equation and solve for ΔG°.