**Matching Reaction Descriptions to Energy Diagrams****Instructions:**Match the description to the letter of the given diagram. [The vertical scales are hard to read, so assume the same scale for all three graphs, i.e., they all go from zero to a maximum free energy of 160 kJ/mole.] Ignore the words at the upper left, including the numbers.**Descriptions:**31. fast exothermic reaction32. slow equilibrium reaction33. slow endothermic reaction**Diagrams and Descriptions:****Diagram A:**This diagram shows a potential energy curve for a reaction path. The curve starts with reactants at a higher energy level, peaks at the activation energy (Ea), and then decreases to a lower energy level at the products stage, indicating an exothermic reaction (shown by ΔH). This suggests a release of energy in the form of heat (exothermic).**Diagram B:**The graph depicts a reaction progress with reactants starting at a lower energy level, reaching a peak at the transition state (activation energy Ea), and then only slightly decreasing energy towards the products. This represents a slow equilibrium reaction, where the difference in energy between reactants and products is minimal, resulting in a slow release of energy.**Diagram C:**This charts the reaction progress from reactants at a lower energy level increasing to the transition state (Ea) and finally to products at a higher energy level, indicating an increase in energy absorption, suggesting an endothermic reaction (energy is absorbed). The notable rise in energy from reactants to products aligns with a slow endothermic process.**Matching Exercise:**For each description, select the corresponding diagram (A, B, or C).- 31. Fast exothermic reaction: Diagram A- 32. Slow equilibrium reaction: Diagram B- 33. Slow endothermic reaction: Diagram C**Answer Section:**(Match the given options to the correct diagrams)- Fast, exergonic: **Diagram A**- Slow, equilibrium: **Diagram B**- Slow, minimal energy released: **Diagram C**- Slow, endergonic: **Diagram C**Ensure to use the additional dropdown options for precise matching.

Match the following description: Fast, exergonic = A Slow, equilibrium = None of these slow, minimal…

Match the description to the letter of the given diagram. [The vertical scales are hard to read, so assume the same scale for all three graphs, i.e., they all go from zero to a maximum free energy of 160 kJ/mole.][And ignore the words at the upper left, including the #s.] 31. fast exothermic reaction 32. slow equilibrium reaction. 33. slow endothermic reaction. B (kJ/mole) All- A activation energy Ea Potential energy reactants (kJ) ΔΗ products reaction pathway Fast, exergonic slow, equilibrium slow, minimal energy released. Slow, endergonic 140 120 200 (kJ/mole) mole Reaction Progress 30. B None of these Not enough information A с Recar Reaction Progress C

Match the description to the letter of the given diagram. [The vertical scales are hard to read, so assume the same scale for all three graphs, i.e., they all go from zero to a maximum free energy of 160 kJ/mole.][And ignore the words at the upper left, including the #s.] 31. fast exothermic reaction 32. slow equilibrium reaction. 33. slow endothermic reaction. B (kJ/mole) All- A activation energy Ea Potential energy reactants (kJ) ΔΗ products reaction pathway Fast, exergonic slow, equilibrium slow, minimal energy released. Slow, endergonic 140 120 200 (kJ/mole) mole Reaction Progress 30. B None of these Not enough information A с Recar Reaction Progress C

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...

See similar textbooks

Similar questions

A spontaneous reaction always releases heat. True False
At 699 K, AG° =-23.25 kJ for the reaction H2( g) + I2( g) + 2HI( g). Calculate AG for this reaction if the reactants are both at 10.0 atm pressure and the product is at 2.27 atm pressure. a. 40.5 kJ O b. 6.0 kJ O c. 17.2 kJ O d.-17.2 kJ e. -40.5 kJ
Energy drives chemical reactions. For a reaction that goes from Y→ X, using Table 3-1 in your book, how many times more [X] than [Y] will there be at equilibrium if the standard free energy change (Gᵒ)for that reaction is -2.8 kcal/mole? a. 10 O b. 1/10 c. 100 d. 10,000 e. Not enough information
If the ΔG'° of the reaction A → B is –40 kJ/mol, under standard conditions the reaction: a. is at equilibrium. b. will never reach equilibrium. c. will not occur spontaneously. d. will proceed at a rapid rate. e. will proceed spontaneously from left to right.
An explanation of how electrons are exchanged between atoms during a chemical reaction would be classified as a(n) a. spontaneous reaction b. activation energy c. reaction rate d. reaction mechanism
Given this reaction at equilibrium, C(s) + CO2(g) D 2CO(g) (∆H° = 119kJ), explain the changes that would occur when the following stresses are applied: a.CO is removed. b.Heat is removed. c.CO2 is added.
In what condition, a reaction is product-favored. Select the correct answer... a. K° = 0 and G° = 0. b. K° < 1 and G° = 0. c. K° < 1 and G° > 0. d. K° > 1 and G° < 0. e. K° = 1 and G° = 0.