Question

Find ΔS° for the formation of 1 mole of Cu2O(s) from its elements. ΔS° = _______ J/K.

Answer 1

To calculate ΔS° for the formation of Cu2O(s), standard molar entropy values for the reactants and product are required, which are typically found in thermodynamic tables.

Step-by-step explanation:

The question asks to find the standard entropy change (ΔS°) for the formation of 1 mole of copper(I) oxide (Cu2O) from its elements. Standard entropy changes can be calculated using standard molar entropy values of products and reactants. Typically, the values are available in standard thermodynamic tables but are not provided in the question. If the standard molar entropies for Cu, O2, and Cu2O were given, the calculation would follow the formula:

ΔS° = ΣS°(products) - ΣS°(reactants)

However, since actual values are not provided, the specific ΔS° for Cu2O cannot be calculated here. One would need the standard molar entropy for solid copper, molecular oxygen, and copper(I) oxide to carry out this calculation.

Answer 2

To find the standard entropy change for the formation of 1 mole of Cu2O(s) from its elements, you need to calculate the difference in entropy between the products and reactants.

Step-by-step explanation:

The question asks for the standard entropy change (∆S°) for the formation of 1 mole of Cu2O(s) from its elements. To find this value, we need to determine the difference in entropy between the products and reactants. The equation for the formation of Cu2O(s) from its elements is:

2Cu(s) + 1/2O2(g) → Cu2O(s)

Using the given entropy values for the elements and compounds at 298 K, we can calculate the standard entropy change:

∆S° = [2S°(Cu2O(s))] - [2S°(Cu(s)) + 1/2S°(O2(g))]