The value of ^G for the following reaction is -5490 kJ. Use this value and data to calculate the standard free energy of formation for C4H10 (g).

2 C4H10 (g) + 13 O2 (g) --> 8 CO2 (g) + 10 H2o (l)

Do you know the heats of formation for CO2 and H2O?

Wouldn't delta G/2, minus 4 Hfco2, minus 5 Hfh2o, equal Hfbutane?

heat of formation for CO2(g) is -393.5 kJ/mol and for H2O(l) it's -285.8 kJ/mol

Ah, I see you're trying to calculate the standard free energy of formation for butane using the given reaction and known heats of formation. Well, I happen to know a thing or two about this!

The heats of formation, denoted by Hf, tell us the amount of energy released or absorbed when one mole of a substance is formed from its constituent elements in their standard states.

To calculate the standard free energy of formation for butane (C4H10), we can use the given reaction and the known heats of formation for CO2 and H2O. However, I must confess, I don't know those specific values off the top of my head. But fret not! Google is your friend in this case.

Now, to address your equation:

ΔG/2 - 4HfCO2 - 5HfH2O = Hfbutane

Roughly speaking, it seems like you're trying to utilize the stoichiometric coefficients from the reaction equation. However, it's important to note that the ΔG value you have (-5490 kJ) is the overall change in free energy for the entire reaction, not just for the formation of butane.

To calculate the standard free energy of formation for butane, you'll need to consider the ΔG value for the complete reaction and use the known heats of formation for CO2 and H2O. Remember to account for the stoichiometric coefficients of each reactant and product in your calculation!

I wish you the best of luck in your thermodynamic endeavors. Remember, humor can be a good way to lighten the mood when dealing with challenging calculations. So, if you need a little break from the numbers, just let me know!

To calculate the standard free energy of formation (ΔGf) for C4H10 (butane), we need to know the heats of formation for CO2 and H2O. These values represent the change in enthalpy when one mole of a substance is formed at standard conditions (1 atm pressure and 25°C temperature).

Let's assume that the given ΔG value of -5490 kJ corresponds to the standard conditions.

The equation you provided is as follows:

2 C4H10 (g) + 13 O2 (g) --> 8 CO2 (g) + 10 H2O (l)

To calculate the standard free energy of formation for C4H10 (ΔGfbutane), we can use the formula:

ΔGfbutane = (ΔG/2) - 4ΔHfCO2 - 5ΔHfH2O

Where:
ΔG/2 is the standard free energy change of the reaction (given as -5490 kJ),
ΔHfCO2 is the heat of formation of CO2,
ΔHfH2O is the heat of formation of H2O,
and ΔGfbutane is the standard free energy of formation for C4H10 (butane) that we want to calculate.

Substituting the given values:

ΔGfbutane = (-5490 kJ/2) - (4 × ΔHfCO2) - (5 × ΔHfH2O)

Since we don't have the heats of formation for CO2 and H2O, we cannot directly calculate the standard free energy of formation for C4H10 using the given information. You would need additional data or previous knowledge of the heats of formation for CO2 and H2O to solve for ΔGfbutane.

To calculate the standard free energy of formation (ΔG°f) for C4H10 (butane), you can use the heat of formation (ΔH°f) values for CO2 and H2O.

Since the reaction equation provided is balanced and involves the formation of 2 moles of butane (C4H10), you need to divide the given ΔG value (-5490 kJ) by 2 to account for the stoichiometry of the reaction.

ΔG°f(C4H10) = ΔG° / 2

Now, to calculate the standard free energy of formation for CO2 and H2O, you would need to use the heat of formation values, denoted as ΔH°f.

ΔG° = ΔH° - TΔS°

In this case, we need to find ΔG°f butane. So the equation becomes:

ΔG°f(C4H10) = ΔH°f(C4H10) - TΔS°f(C4H10)

To proceed, you would need to know the heats of formation for CO2 (ΔH°f(CO2)) and H2O (ΔH°f(H2O)). If you have those values, you can proceed with the calculation.

Regarding your equation "ΔG/2 - 4Hf(CO2) - 5Hf(H2O) = Hf(butane)", it seems that you are attempting to use Hess's law to relate the ΔG values, the heats of formation, and the formation of butane. However, this equation is not accurate. To obtain the standard free energy of formation of butane, you would need to use the equation mentioned above and the known ΔH°f values for CO2 and H2O.