Question

Chemical thermodynamics"

Calculate A,H, A,S, and A,G using the following reaction:

MgCO3(s) + 2 HCl (1)→ MgCl2(s) + H2O(1)

Calculate the Gibbs energy and determine whether the reaction can proceed at temperatures of 293 and 1293 Κ.

Variant 19

Answer 1

The spontaneity of the reaction 2 H2(g) + O2(g) → 2 H2O(g) can be assessed by calculating the Gibbs free energy change.

Step-by-step explanation:

To determine if the reaction (2 H₂(g) + O₂(g) → 2 H₂O(g)) proposed by Professor Nesral is spontaneous, we need to calculate the Gibbs free energy change (ΔG) at a given temperature. The Gibbs free energy change is given by the equation ΔG = ΔH - TΔS where ΔH is the enthalpy change, T is the temperature in kelvins, and ΔS is the entropy change. For a reaction happening under standard conditions, we use ΔG°, ΔH°, and ΔS°, which are the standard changes in Gibbs energy, enthalpy, and entropy, respectively.

To calculate ΔG° at 298 K for the combustion of hydrogen, we would need the standard enthalpy change (ΔH°) and the standard entropy change (ΔS°) for the reaction, which can be found in thermodynamic tables.

Without the specific values of ΔH° and ΔS°, we can't calculate the exact ΔG° for the reaction. However, we know that the combustion of hydrogen is typically exothermic (releasing heat, ΔH° < 0) and leads to an increase in disorder (positive ΔS°), suggesting that the reaction is indeed spontaneous under standard conditions (ΔG° < 0). At higher temperatures, the value of TΔS becomes larger, which could potentially make ΔG even more negative, thus supporting the spontaneity of the reaction at 330 K in El Azizia, Libya as well.