Calculate Delta G for The Following Reaction 9no

What is ΔG?

ΔG (Gibbs free energy change) is a thermodynamic property that measures the energy available to do work in a system. It's calculated using the formula:

Where:

• ΔG = Gibbs free energy change (kJ/mol)
• ΔH = Enthalpy change (kJ/mol)
• T = Absolute temperature (K)
• ΔS = Entropy change (J/mol·K)

The sign of ΔG determines the spontaneity of a reaction:

• ΔG < 0: Reaction is spontaneous
• ΔG = 0: Reaction is at equilibrium
• ΔG > 0: Reaction is non-spontaneous

How to calculate ΔG

To calculate ΔG for the reaction 9NO, you'll need:

1. The standard enthalpy change (ΔH°) for the reaction
2. The standard entropy change (ΔS°) for the reaction
3. The temperature at which the reaction occurs

The calculation follows the standard Gibbs free energy equation:

Where ΔG° represents the standard Gibbs free energy change.

Standard conditions

Standard conditions for ΔG calculations are:

• Temperature: 298 K (25°C)
• Pressure: 1 atm
• Concentration: 1 M for solutes

Standard conditions provide a consistent reference point for comparing reactions.

Reaction spontaneity

The spontaneity of a reaction is determined by the sign of ΔG:

• If ΔG is negative, the reaction will proceed spontaneously
• If ΔG is positive, the reaction will not proceed spontaneously
• If ΔG is zero, the reaction is at equilibrium

Understanding spontaneity helps predict reaction behavior and design chemical processes.

Example calculation

Let's calculate ΔG for the reaction 9NO under standard conditions:

1. Given ΔH° = -180.5 kJ/mol
2. Given ΔS° = -240 J/mol·K
3. Temperature T = 298 K

Using the formula:

First convert ΔS to kJ/mol·K:

Now calculate:

The negative ΔG indicates this reaction is spontaneous under standard conditions.