Question

Calculate ΔS∘rxn for the following reaction. The ΔS∘ for each species is shown below the reaction.

C2H2(g) + 2H2(g) → C2H6(g)
S∘(J/mol⋅K) 200.9 130.7 229.2

A) -159.0 J/K
B) -233.1 J/K
C) +233.1 J/K
D) 303.3 J/K
E) 560.8 J/K

Answer 1

Answer:

-233.1 J/K

Explanation:

Answer 2

The standard entropy change for the reaction C₂H₂(g) + 2 H₂(g) → C₂H₆(g), is B) -233.1 J/K.

Let's consider the following balanced equation.

C₂H₂(g) + 2 H₂(g) → C₂H₆(g)

Entropy is a measure of how much the energy of atoms and molecules becomes more spread out in a process. We can calculate the standard entropy change for the reaction (ΔS°rxn) using the following expression.

$\Delta S \°_{rxn} = \Sigma n_p \times S_p\° - \Sigma n_r \times S_r\°$

where,

• n: moles
• S°: standard entropy of the species
• p: products
• r: reactants

$\Delta S \°_{rxn} = 1 mol \times S\°(C_2H_6) - 1 mol \times S\°(C_2H_2) - 2 mol \times S\°(H_2)\\\Delta S \°_{rxn} = 1 mol \times (229.2J/mol.K) - 1 mol \times (200.9J/K.mol) - 2 mol \times (130.7J/K.mol) = -233.1 J/K$

The standard entropy change for the reaction C₂H₂(g) + 2 H₂(g) → C₂H₆(g), is B) -233.1 J/K.

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