The equation for the formation of silicon tetrachloride from silicon and chlorine is Si(s) + 2Cl 2 (g) → SiCl 4 (g) + 657 kJ b. Is the energy of the product higher or lower than the energy of the reactants?

Welcome back, everyone. The reaction between silicon and fluorine produces silicon tetra fluoride as shown below, determine whether the energy of the products is lower or higher than that of the reactants. We're going to observe that in our given equation, not only do we have on our product side, our gaseous silicon tetra fluoride as a product, but we also have the figure plus 1615 kilojoules of heat that is released. So we're going to interpret that from this figure. Therefore, we have an exothermic reaction which is defined as a reaction where the energy of our reactant is greater than the energy of our products allowing for a negative entropy change. Negative delta H which describes the heat content of our system being our reaction. And with a negative entropy change, we understand that we have an exothermic process, which is why we next want to recall that for an exothermic reaction, we would observe a bond formation of our products which corresponds to the release of heat and a decrease in energy of our system. But an increase in energy for our surroundings, which corresponds to an increase in temperature of our surroundings. And as we stated earlier, an exothermic reaction is characterized by a negative entropy change due to the fact that the energy of our reactants is greater than the energy of our products. So, based on everything we've outlined, we can determine that because we have an exothermic reaction releasing 1615 kilojoules of heat. Therefore, our energy of our products will be lower than the energy of our reactants. So this is our final answer. I hope this made sense and let us know if you have any questions.

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7. Energy, Rate and Equilibrium

Endothermic & Exothermic Reactions

GOB Chemistry

7. Energy, Rate and Equilibrium

Endothermic & Exothermic Reactions

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Problem 107b

Textbook Question

The equation for the formation of silicon tetrachloride from silicon and chlorine is Si(s) + 2Cl₂(g) → SiCl₄(g) + 657 kJ
b. Is the energy of the product higher or lower than the energy of the reactants?

Verified step by step guidance

Step 1: Begin by analyzing the chemical equation provided: Si(s) + 2Cl₂(g) → SiCl₄(g) + 657 kJ. The '+ 657 kJ' indicates that energy is released during the reaction, which classifies this as an exothermic reaction.

Step 2: Recall the concept of energy changes in chemical reactions. In an exothermic reaction, the energy of the products is lower than the energy of the reactants because energy is released to the surroundings.

Step 3: Understand that the energy released (657 kJ) represents the difference between the energy of the reactants and the energy of the products. This means the reactants had higher energy initially, and the products have lower energy after the reaction.

Step 4: Conclude that the energy of the product, SiCl₄(g), is lower than the energy of the reactants, Si(s) and Cl₂(g), due to the release of 657 kJ of energy.

Step 5: To reinforce understanding, consider the energy diagram for an exothermic reaction: the reactants start at a higher energy level, and the products end at a lower energy level, with the difference in energy released as heat.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Exothermic Reactions

An exothermic reaction is a chemical reaction that releases energy in the form of heat or light. In the given equation, the formation of silicon tetrachloride from silicon and chlorine releases 657 kJ, indicating that the products have lower energy than the reactants. This energy release is a key characteristic of exothermic processes.

Enthalpy Change

Enthalpy change (ΔH) refers to the heat content of a system at constant pressure. In the context of the reaction provided, the negative value of ΔH (−657 kJ) signifies that the products (SiCl4) have a lower enthalpy than the reactants (Si and Cl2). Understanding enthalpy changes helps in predicting the energy dynamics of chemical reactions.

Thermodynamics

Thermodynamics is the branch of physical science that deals with the relationships between heat, work, temperature, and energy. It provides the framework for understanding how energy is transferred in chemical reactions. In this case, thermodynamic principles explain why the energy of the products is lower than that of the reactants, as energy is released during the formation of SiCl4.

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The equation for the formation of silicon tetrachloride from silicon and chlorine is Si(s) + 2Cl2(g) → SiCl4(g) + 657 kJ b. Is the energy of the product higher or lower than the energy of the reactants?

Key Concepts

Exothermic Reactions

Enthalpy Change

Thermodynamics

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The equation for the formation of silicon tetrachloride from silicon and chlorine is Si(s) + 2Cl₂(g) → SiCl₄(g) + 657 kJ
b. Is the energy of the product higher or lower than the energy of the reactants?