For the reaction C2 H2(g)+4 F2(g) ⟶2 CF4(g)+H2(g) ΔS^∘ is equal to -358 J / K. Use this value

step 1 answer for the problem here we have to find the change in entropy so we have a reaction is c2 h2

For the reaction C2 H2(g)+4 F2(g) ⟶2 CF4(g)+H2(g) ΔS^∘ is...

For the reaction $$\mathrm{C}_{2} \mathrm{H}_{2}(g)+4 \mathrm{~F}_{2}(g) \longrightarrow 2 \mathrm{CF}_{4}(g)+\mathrm{H}_{2}(g) $$$\Delta S^{\circ}$ is equal to $-358 \mathrm{~J} / \mathrm{K}$. Use this value and data from Appendix 4 to calculate the value of $S^{\circ}$ for $\mathrm{CF}_{4}(g)$.

For the reaction
$$\mathrm{C}_{2} \mathrm{H}_{2}(g)+4 \mathrm{~F}_{2}(g) \longrightarrow 2 \mathrm{CF}_{4}(g)+\mathrm{H}_{2}(g)
$$$\Delta S^{\circ}$ is equal to $-358 \mathrm{~J} / \mathrm{K}$. Use this value and data from Appendix 4 to calculate the value of $S^{\circ}$ for $\mathrm{CF}_{4}(g)$.

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Key Concepts

Standard Molar Entropy

Standard molar entropy is a measure of the absolute entropy of one mole of a substance under standard conditions. It provides insight into the degree of randomness or disorder present in a substance at a specified temperature (usually 298 K) and pressure. These values are fundamental for calculating the overall entropy changes in chemical reactions.

Entropy Change of Reaction

The entropy change of a reaction (?S°) is determined by the difference between the total standard molar entropies of the products and the reactants, each multiplied by their respective stoichiometric coefficients. This concept helps in understanding how the disorder of a system changes during a chemical transformation and is crucial for assessing the spontaneity of a reaction.

Thermodynamic Data Tables

Thermodynamic data tables provide standard values for properties like standard molar entropy, enthalpy, and Gibbs free energy of substances under standard conditions. These tables are essential tools in thermodynamics, allowing scientists to perform calculations and predict the behavior of chemical reactions by accessing consistent and reliable reference data.

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