Does the reaction P4(s, white) + 5 O2(g) P4O10(s) occur spontaneously at 298 K and standard state conditions?

Calculate the value of capital delta S°univ.

Honestly do not know where to start.

To determine whether the reaction occurs spontaneously at 298 K and standard state conditions, you need to calculate the Gibbs free energy change (ΔG°) for the reaction.

The Gibbs free energy change can be determined using the formula:

ΔG° = ΔH° - TΔS°

Where:
ΔG° is the Gibbs free energy change
ΔH° is the enthalpy change
T is the temperature in Kelvin
ΔS° is the entropy change

Step 1: Find ΔH°
You will need the enthalpy of formation for each compound involved in the reaction. Look up the values in a reliable source such as a chemistry handbook or database.

ΔH° for the reaction can be calculated as:
ΔH° = Σ (ΔH°f products) - Σ (ΔH°f reactants)

Step 2: Find ΔS°
You will need the entropy change for each compound involved in the reaction. Again, refer to a reliable source for the necessary values.

ΔS° for the reaction can be calculated as:
ΔS° = Σ (ΔS° products) - Σ (ΔS° reactants)

Step 3: Calculate ΔG°
Plug the values of ΔH° and ΔS° into the formula:
ΔG° = ΔH° - TΔS°

It is important to note that standard state conditions assume a pressure of 1 atmosphere and concentrations of 1 Molar for all reactants and products.

After calculating ΔG°, evaluate its sign:
- If ΔG° is negative, the reaction occurs spontaneously.
- If ΔG° is positive, the reaction does not occur spontaneously.
- If ΔG° is zero, the system is at equilibrium.

Please note that the equilibrium constant, K, can also be used to determine spontaneity. If K is greater than 1, the reaction is spontaneous; if K is less than 1, the reaction is non-spontaneous.

dSo system = (n*dSo formation products) - (n*dSo formation reactants)

dHo system = (n*dHo formation products) - (n*dHo reactants)
dSo surroundings = -dHosystem/T

Plug dSo surroundings and dSo system into the following and solve for dSo universe.
dSouniverse = dSosystem + dSosurroundings