Ethylene gas and steam at 593.15 K(320^∘ C) and atmospheric pressure are fed to a reaction proc

step 1 In this question we are looking into the reaction where C2H4 is reacting with H2O to produce CH3

Ethylene gas and steam at 593.15 K(320^∘ C) and atmospheric...

Ethylene gas and steam at $593.15 \mathrm{~K}\left(320^{\circ} \mathrm{C}\right)$ and atmospheric pressure are fed to a reaction process as an equimolar mixture. The process produces ethanol by the reaction: $$ \mathrm{C}_2 \mathrm{H}_4(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}(l) $$ The liquid ethanol exits the process at $298.15 \mathrm{~K}\left(25^{\circ} \mathrm{C}\right)$. What is the heat transfer associated with this overall process per mole of ethanol produced?

Ethylene gas and steam at $593.15 \mathrm{~K}\left(320^{\circ} \mathrm{C}\right)$ and atmospheric pressure are fed to a reaction process as an equimolar mixture. The process produces ethanol by the reaction:
$$
\mathrm{C}_2 \mathrm{H}_4(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}(l)
$$

The liquid ethanol exits the process at $298.15 \mathrm{~K}\left(25^{\circ} \mathrm{C}\right)$. What is the heat transfer associated with this overall process per mole of ethanol produced?

Key Concepts

Enthalpy of Reaction

This concept involves determining the overall heat exchange during a chemical reaction. It is based on the difference between the enthalpies of the products and the reactants and can be calculated using standard enthalpies of formation or through Hess’s law. It provides the basis for understanding whether a reaction is exothermic or endothermic and quantifies the thermal energy released or absorbed during the transformation.

Hess’s Law

Hess’s Law states that the total enthalpy change for a reaction is independent of the pathway taken, as long as the initial and final conditions are the same. This principle allows complex processes involving multiple steps—which may include phase changes and temperature variations—to be analyzed by breaking them down into simpler, more easily tabulated steps, and then summing their enthalpy changes.

Sensible Heat and Heat Capacity

Sensible heat refers to the energy involved in changing the temperature of a substance without a phase change. The amount of energy required to raise or lower the temperature of a substance is determined by its heat capacity. In processes that involve cooling or heating the reactants and products from one temperature to another, the calculation of sensible heat is critical to the overall energy balance.

Phase Change Enthalpy

When a substance undergoes a phase change, such as condensation or vaporization, latent heat is absorbed or released without changing temperature. This concept is essential for understanding processes where the physical state of a reactant or product changes, as the latent heat associated with these transitions significantly affects the total heat transfer in the process.

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