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Ch.14 - Chemical Kinetics
Chapter 14, Problem 95b

Consider this energy diagram:
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b. Label the reactants, products, and intermediates.

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1
Step 1: Understand the components of an energy diagram. An energy diagram typically shows the energy changes during a chemical reaction, with the y-axis representing energy and the x-axis representing the reaction progress.
Step 2: Identify the starting point of the diagram. The reactants are usually located at the beginning of the energy diagram, where the reaction starts.
Step 3: Locate the ending point of the diagram. The products are found at the end of the energy diagram, where the reaction concludes.
Step 4: Look for any peaks or valleys between the reactants and products. These represent intermediates or transition states, which are temporary species formed during the reaction.
Step 5: Label the diagram accordingly. Mark the initial energy level as 'Reactants', the final energy level as 'Products', and any intermediate peaks or valleys as 'Intermediates'.

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Related Practice
Open Question
The reaction AB(aq) → A(g) + B(g) is second order in AB and has a rate constant of 0.0118 M^-1 s^-1 at 25.0 °C. A reaction vessel initially contains 250.0 mL of 0.100 M AB that is allowed to react to form the gaseous product. The product is collected over water at 25.0 °C. How much time is required to produce 200.0 mL of the products at a barometric pressure of 755.1 mmHg? (The vapor pressure of water at this temperature is 23.8 mmHg.)
Open Question
The reaction 2 H2O2(aq) → 2 H2O(l) + O2(g) is first order in H2O2 and under certain conditions has a rate constant of 0.00752 s⁻¹ at 20.0 °C. A reaction vessel initially contains 150.0 mL of 30.0% H2O2 by mass solution (the density of the solution is 1.11 g/mL). The gaseous oxygen is collected over water at 20.0 °C as it forms. What volume of O2 forms in 85.0 seconds at a barometric pressure of 742.5 mmHg? (The vapor pressure of water at this temperature is 17.5 mmHg.)
Textbook Question

Consider this energy diagram:

a. How many elementary steps are involved in this reaction?

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Textbook Question

Consider this energy diagram:

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c. Which step is rate limiting?

Textbook Question

Consider this energy diagram:

d. Is the overall reaction endothermic or exothermic?

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Open Question
Is the overall reaction exothermic or endothermic in the mechanism where HCl adds across the double bond of ethene to form H3C¬CH2Cl, with the energy diagram indicating step 1 as HCl + H2C“CH2 → H3C“CH2+ + Cl⁻ and step 2 as H3C“CH2+ + Cl⁻ → H3C¬CH2Cl?