QUESTION 3 In Chem 113, we saw that the heat associated with a chemical reaction could be determined in one step, or as the sum of two steps, as long as the two steps resulted in the same overall reaction. (Hess' Law). Consider a reaction which occurs in the two steps shown below. What is the overall reaction that these two steps are equivalent to? Step 1: H202(aq) + I(aq) --> H2O + Or-(aq) Step 2: H202(aq) + O1-(aq) - H20 + 02(g) - I(aq)
QUESTION 3 In Chem 113, we saw that the heat associated with a chemical reaction could be determined in one step, or as the sum of two steps, as long as the two steps resulted in the same overall reaction. (Hess' Law). Consider a reaction which occurs in the two steps shown below. What is the overall reaction that these two steps are equivalent to? Step 1: H202(aq) + I(aq) --> H2O + Or-(aq) Step 2: H202(aq) + O1-(aq) - H20 + 02(g) - I(aq)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
![**Chemical Reactions Involving Hydrogen Peroxide**
Below are different chemical equations showcasing various reactions involving hydrogen peroxide (\( \text{H}_2\text{O}_2 \)) in aqueous solution. Each equation includes the initial reactants, the resultant products, and their respective states (aqueous or gaseous).
**a.**
\[
2 \, \text{H}_2\text{O}_2(aq) \rightarrow 2 \, \text{H}_2\text{O}(l) + \text{O}_2(g)
\]
This equation represents the decomposition of hydrogen peroxide into water and oxygen gas.
**b.**
\[
\text{H}_2\text{O}_2(aq) + \text{OI}^-(aq) + \text{I}^-(aq) \rightarrow \text{H}_2\text{O}(l) + \text{O}_2(g) + \text{I}_2(g)
\]
In this reaction, hydrogen peroxide reacts with hypoiodite (\( \text{OI}^- \)) and iodide ions (\( \text{I}^- \)) to form water, oxygen gas, and iodine gas.
**c.**
\[
2 \, \text{H}_2\text{O}_2(aq) + 2 \, \text{I}^-(aq) \rightarrow 2 \, \text{H}_2(g) + 2 \, \text{O}_2(g) + \text{I}_2(aq)
\]
Hydrogen peroxide reacts with iodide ions to form hydrogen gas, oxygen gas, and aqueous iodine.
**d.**
\[
2 \, \text{H}_2\text{O}_2(aq) + 2 \, \text{OI}^-(aq) \rightarrow 2 \, \text{H}_2(g) + 3 \, \text{O}_2(g) + 2 \, \text{I}^-(aq)
\]
This equation shows hydrogen peroxide reacting with hypoiodite ions to produce hydrogen gas, oxygen gas, and iodide ions in solution.
Each equation illustrates different chemical pathways and products that can result from reactions involving hydrogen peroxide, emphasizing its role as an oxidizing and reducing agent.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F07e9effc-21af-434f-b1d9-5938ea63da08%2F9ebebe8b-5edc-4e7f-b30b-57fced7c092c%2Fbfk9e67_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Reactions Involving Hydrogen Peroxide**
Below are different chemical equations showcasing various reactions involving hydrogen peroxide (\( \text{H}_2\text{O}_2 \)) in aqueous solution. Each equation includes the initial reactants, the resultant products, and their respective states (aqueous or gaseous).
**a.**
\[
2 \, \text{H}_2\text{O}_2(aq) \rightarrow 2 \, \text{H}_2\text{O}(l) + \text{O}_2(g)
\]
This equation represents the decomposition of hydrogen peroxide into water and oxygen gas.
**b.**
\[
\text{H}_2\text{O}_2(aq) + \text{OI}^-(aq) + \text{I}^-(aq) \rightarrow \text{H}_2\text{O}(l) + \text{O}_2(g) + \text{I}_2(g)
\]
In this reaction, hydrogen peroxide reacts with hypoiodite (\( \text{OI}^- \)) and iodide ions (\( \text{I}^- \)) to form water, oxygen gas, and iodine gas.
**c.**
\[
2 \, \text{H}_2\text{O}_2(aq) + 2 \, \text{I}^-(aq) \rightarrow 2 \, \text{H}_2(g) + 2 \, \text{O}_2(g) + \text{I}_2(aq)
\]
Hydrogen peroxide reacts with iodide ions to form hydrogen gas, oxygen gas, and aqueous iodine.
**d.**
\[
2 \, \text{H}_2\text{O}_2(aq) + 2 \, \text{OI}^-(aq) \rightarrow 2 \, \text{H}_2(g) + 3 \, \text{O}_2(g) + 2 \, \text{I}^-(aq)
\]
This equation shows hydrogen peroxide reacting with hypoiodite ions to produce hydrogen gas, oxygen gas, and iodide ions in solution.
Each equation illustrates different chemical pathways and products that can result from reactions involving hydrogen peroxide, emphasizing its role as an oxidizing and reducing agent.
![**Question 3**
In Chem 113, we saw that the heat associated with a chemical reaction could be determined in one step, or as the sum of two steps, as long as the two steps resulted in the same overall reaction. This concept is known as Hess's Law.
Consider a reaction which occurs in the two steps shown below. What is the overall reaction that these two steps are equivalent to?
**Step 1:**
\[\text{H}_2\text{O}_2(\text{aq}) + \text{I}^- (\text{aq}) \rightarrow \text{H}_2\text{O} + \text{OI}^- (\text{aq})\]
**Step 2:**
\[\text{H}_2\text{O}_2(\text{aq}) + \text{OI}^- (\text{aq}) \rightarrow \text{H}_2\text{O} + \text{O}_2(\text{g}) + \text{I}^- (\text{aq})\]
Determine the overall reaction that these two steps are equivalent to.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F07e9effc-21af-434f-b1d9-5938ea63da08%2F9ebebe8b-5edc-4e7f-b30b-57fced7c092c%2Frhe6qpt_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question 3**
In Chem 113, we saw that the heat associated with a chemical reaction could be determined in one step, or as the sum of two steps, as long as the two steps resulted in the same overall reaction. This concept is known as Hess's Law.
Consider a reaction which occurs in the two steps shown below. What is the overall reaction that these two steps are equivalent to?
**Step 1:**
\[\text{H}_2\text{O}_2(\text{aq}) + \text{I}^- (\text{aq}) \rightarrow \text{H}_2\text{O} + \text{OI}^- (\text{aq})\]
**Step 2:**
\[\text{H}_2\text{O}_2(\text{aq}) + \text{OI}^- (\text{aq}) \rightarrow \text{H}_2\text{O} + \text{O}_2(\text{g}) + \text{I}^- (\text{aq})\]
Determine the overall reaction that these two steps are equivalent to.
Expert Solution
Step 1
Multistep reactions are those reactions that occur in more than one step.
To get an overall reaction, every step must be added.
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