Calculate the DELTA H(rxn), DELTA S(rxn), DELTA S(universe), DELTA G(rxn). For each system below indicate whether DELTA S and DELTA H are positive or negative. Then indicate if the reaction is entropy driven, enthalpy driven or neither.

C3H8(g) + 2O2(g) => 3CO2(g) + 4H2O(g)

To calculate the values of ΔH, ΔS, ΔS(universe), and ΔG for the given reaction:

1. Determine the number of moles of each substance involved in the reaction:
C3H8(g): 1 mole
O2(g): 2 moles
CO2(g): 3 moles
H2O(g): 4 moles

2. Look up the standard enthalpy of formation (ΔH°f) values for each substance involved in the reaction. These values represent the change in enthalpy when 1 mole of the compound is formed from its constituent elements at standard conditions (25°C and 1 atm).

The standard enthalpy of formation values are as follows:
ΔH°f(C3H8) = -103.8 kJ/mol
ΔH°f(O2) = 0 kJ/mol
ΔH°f(CO2) = -393.5 kJ/mol
ΔH°f(H2O) = -241.8 kJ/mol

3. Calculate ΔH(rxn):
ΔH(rxn) = (ΣΔH°f(products)) - (ΣΔH°f(reactants))
ΔH(rxn) = [(3 mol)(-393.5 kJ/mol) + (4 mol)(-241.8 kJ/mol)] - [(1 mol)(-103.8 kJ/mol) + (2 mol)(0 kJ/mol)]
ΔH(rxn) = -2219.9 kJ/mol - (-103.8 kJ/mol)
ΔH(rxn) = -2116.1 kJ/mol

4. Determine the sign of ΔH(rxn):
ΔH(rxn) is negative (-2116.1 kJ/mol). Therefore, ΔH is negative.

5. Calculate ΔS(rxn):
ΔS(rxn) = (Σn(products) x S°(products)) - (Σn(reactants) x S°(reactants))

The standard entropy (S°) values for each substance involved in the reaction are:
S°(C3H8) = 269.9 J/(mol·K)
S°(O2) = 205.03 J/(mol·K)
S°(CO2) = 213.7 J/(mol·K)
S°(H2O) = 188.7 J/(mol·K)

ΔS(rxn) = [(3 mol)(213.7 J/(mol·K)) + (4 mol)(188.7 J/(mol·K))] - [(1 mol)(269.9 J/(mol·K)) + (2 mol)(205.03 J/(mol·K))]
ΔS(rxn) = 1019.9 J/(mol·K) - 680.96 J/(mol·K)
ΔS(rxn) = 338.93 J/(mol·K)

6. Determine the sign of ΔS(rxn):
ΔS(rxn) is positive (338.93 J/(mol·K)). Therefore, ΔS is positive.

7. Calculate ΔS(universe):
ΔS(universe) = ΔS(sys) + ΔS(surr)
ΔS(universe) = ΔS(rxn) + ΔS(surr)

Since the reaction involves the formation of more moles of gas (from 3 moles of CO2 and 4 moles of H2O) compared to the reactants (1 mole of C3H8 and 2 moles of O2), the change in entropy for the surroundings (ΔS(surr)) is positive.

Therefore, ΔS(universe) > ΔS(rxn).

However, since ΔS sys is positive and ΔS surr is positive but smaller than ΔS sys, the overall ΔS universe is positive but reduced.

8. Determine if the reaction is entropy-driven, enthalpy-driven, or neither:
- ΔS is positive, indicating an increase in disorder or randomness.
- ΔH is negative, indicating the release of heat or energy.

Considering the above information, the given reaction is entropy-driven.

To calculate the delta H(rxn), delta S(rxn), delta S(universe), and delta G(rxn) for the given reaction, we need the standard enthalpy and entropy values for each species involved. These values can be found in thermodynamic data tables or databases.

1. Delta H(rxn) (Change in Enthalpy):
Delta H(rxn) can be calculated by subtracting the sum of the standard enthalpies of the reactants from the sum of the standard enthalpies of the products.
Delta H(rxn) = (3 * Delta Hf(CO2) + 4 * Delta Hf(H2O)) - (Delta Hf(C3H8) + 2 * Delta Hf(O2))

2. Delta S(rxn) (Change in Entropy):
Delta S(rxn) is calculated similarly to delta H, but using the standard entropy values instead of enthalpy values.
Delta S(rxn) = (3 * Delta S(CO2) + 4 * Delta S(H2O)) - (Delta S(C3H8) + 2 * Delta S(O2))

3. Delta S(universe) (Change in Total Entropy):
Delta S(universe) is the sum of the entropy changes of the system and surroundings.
Delta S(universe) = Delta S(rxn) + Delta S(surr)

4. Delta G(rxn) (Change in Free Energy):
Delta G(rxn) can be calculated using the equation:
Delta G(rxn) = Delta H(rxn) - T * Delta S(rxn)
where T is the temperature in Kelvin.

Now, to determine the signs and driving forces:

- If Delta H(rxn) is positive, the reaction is endothermic (enthalpy increases).
- If Delta H(rxn) is negative, the reaction is exothermic (enthalpy decreases).
- If Delta S(rxn) is positive, the reaction is entropy-driven (entropy increases).
- If Delta S(rxn) is negative, the reaction is enthalpy-driven (entropy decreases).

By comparing the signs of Delta H and Delta S, we can determine the driving force of the reaction.

Please note that specific values of enthalpy and entropy for each species are needed to perform the full calculation.

You need to look in your text for a set of thermodynamic tables and apply the following:

delta H(rxn) = delta H products - delta H reactants.
delta S(rxn) = delta S products - delta H reactants.
Then delta G = delta H - T*delta S.