For a particular reaction, Δ H = 120.5 kJ / mol and Δ S = 758.2 J / ( mol⋅K). Calculate Δ G for this reaction at 298 K. Δ G = kJ / mol What can be said about the spontaneity of the reaction at 298 K? The system is at equilibrium. The system is spontaneous in the reverse direction. The system is spontaneous as written.

ΔG = -105.4 kJ/mol

The system is spontaneous as written.

Explanation:

Step 1: Determine Gibbs free energy of reaction (ΔG)

We use the following expression.

ΔG = ΔH - T × ΔS

where,

ΔG = ΔH - T × ΔS

ΔG = 120.5 kJ/mol - 298 K × 0.7582 kJ/mol.K

ΔG = -105.4 kJ/mol

Step 2: Determine the spontaneity of the system.

Since ΔG < 0, the system is spontaneous as written.

you need to take a look at the periodic system in order to sort these elements into pairs that would most likely exhibit similar chemical properties. first, you need to find elements that are found in the same group (groups are vertical in the periodic system), and then to see whether they have the same valence number. if they meet these criteria, they will have similar properties.

the first pair: ne (neon) and kr (krypton), are noble gases found in group 8

the second pair: li (lithium) and k (potassium), found in group 1

the third pair: s (sulfur) and te (tellurium), found in group 6