6. Reaction: 4 NO(g) + 6 H2O(1) - 4 NH3 (g) + 5 O2(g) AHxn° = ( +) a. Based on the probability of particle distribution, which state (reactants or products) is more likely? Explain. b. Is this reaction exothermic or endothermic? Then, based on the probability of thermal energy distribution, do you think the forward or reverse reaction is more likely? Explain. c. Based on your answers to parts a. and b., can you predict which state (reactants or products) is more likely? If not, why not? In either case, explain your thinking!

6. Reaction: 4 NO(g) + 6 H2O(1) - 4 NH3 (g) + 5 O2(g) AHxn° = ( +) a. Based on the probability of particle distribution, which state (reactants or products) is more likely? Explain. b. Is this reaction exothermic or endothermic? Then, based on the probability of thermal energy distribution, do you think the forward or reverse reaction is more likely? Explain. c. Based on your answers to parts a. and b., can you predict which state (reactants or products) is more likely? If not, why not? In either case, explain your thinking!

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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3. In the following reaction, energy is given off. Where does the energy go? 2 C(s) + O₂(g) = 2 CO(g) a. To the reactants b. To the products c. To the system d. To the surroundings
Predict whether the following reactions will be exothermic or endothermic. A. N2(g)+3H2(g)⟶2NH3(g)N2⁡(g)+3⁢H2⁡(g)⟶2⁢NH3⁢(g) B. S(g)+O2(g)⟶SO2(g)S(g)+O2⁡(g)⟶SO2⁢(g) C. 2H2O(g)⟶2H2(g)+O2(g)2⁢H2O(g)⟶2⁢H2⁡(g)+O2⁡(g) D. 2F(g)⟶F2(g)2F(g)⟶F2⁡(g) Bond ??Δ⁢H (kJ/mol) H−HH−H 432 N≡NN≡N 942 O=OO=O 494 F−FF−F 155 H−NH−N 386 H−OH−O 459 S=OS=O 522 S−OS−O 355
13. Energy is stored in the body in adenosine triphosphate, ATP, which is formed by reaction between adenosine diphosphate, ADP, and dihydrogen phosphate ions. ADP3-(aq) + H2PO42-(aq) -----> ATP4-(aq) + H2O (l) ΔH° = 38 kJ Is the reaction endothermic or exothermic?
c. Draw a potential energy diagram for the formation of NO₂(g): N₂(g) +20₂(g) → 2NO2(g). AHreaction = 66.2 kJ/mol. Label the graph with "Reactants," "Products," "AHreaction," and "Ea
During an experiment a student mixed two chemicals together and noted that the beaker felt warm to the touch after the reaction was complete. In the experiment, the chemicals would be classified as the From this observation, the student concluded that the reaction was A. Which of the following energy pathway diagrams represents the chemical reaction from the student's experiment? Ep (kJ) Select one: OA OB 150 125 100 + and the beaker would be classified as the Reaction Coordinate and that the resulting change in enthalpy (AH) would have a B. 125 E 100 Reaction Coordinate Ep (kJ) 150 ◆ value.
6. In a study of glass etching, a chemist examines the reaction between sand (SiO₂) and hydrogen fluoride at 150°C: SiO₂ (s) + 4HF(g) SiF4(g) + 2H₂O(g) Predict the effect on [SiF4] when (a) H₂O(g) is removed; (b) some liquid water is added; (c) HF is removed; (d) some sand is removed.
A reaction is endothermic. If we add heat to the reaction, will it shift to the right (towards products) or to the left (towards reactants)? ?+ℎ???↔?+?
Consider the reaction. 2 Fe₂0₂4Fe +30₂ AHin = +824.2 kJ The formation of 62.0 g of Fe results in the release of 229 kJ of heat. the absorption of 229 kJ of heat. O the release of 12800 kJ of heat. the release of 915 kJ of heat. the absorption of 12800 kJ of heat. the absorption of 915 kJ of heat.
Which of the following statements about the storage of energy using chemical systems are correct? Mark all that are true. A. When energy is stored in a system where Q > K, energy is released from storage when the forward reaction occurs. B. Storing energy in a chemical system requires taking the system away from equilibrium. C. If AG° is negative, the forward reaction will always release energy and the reverse reaction will always store energy. D. The energy available by carrying out the forward reaction will change unless we take some additional action to hold Q constant.
Multiple Choice 1. When a match is lit, the air around the flame feels hot to the hand. Which statement best describes this observation? Heat is absorbed from the system, so it feels hotter. b. The reaction is endothermic. а. The potential energy of the match decreased. d. 3P6) + 10KCIO3 (5) → ЗРо + 10KCIO; (9) — с. 3P,O10 (9) + 10KCI + 9484 kJ 3P,O10 (6) AH = 3161 kJ/mol P е. (s) To answer questions 2 & 3, refer to the following information: A. synthesis reaction B. boiling a liquid C. subliming a solid D. dissolving a solute E. nuclear fission 2. Which of the following is always an example of an exothermic reaction? а. A d. D b. е. Е с. С 3. Which of the following would most likely have the smallest magnitude of enthalpy change? а. A d. B, C and D b. В е. А, В, С, D с. Е 4. How much energy is released when the temperature of 10.6 kg mass of a substance decreases by 15°C, if the substance has a specific heat of 1.6J/g°C? a. 0.10 kJ b. 0.25 kJ c. 0.51 kJ d. 1.0 x 10² kJ е. 250 k]
Consider the reaction. 2 Fe,O, 4 Fe + 30, AHn = +824.2 kJ The formation of 84.0 g of Fe results in the absorption of 3.10 x 102 kJ of heat. the absorption of 17300 kJ heat. the absorption of 1240 kJ of heat. the release of 1240 kJ of heat. the release of 3.10 x 10² kJ of heat. the release of 17300 kJ of heat. G Search or type URL
Indicate whether each of the following reactions is endothermic or exothermic. K*(g) + Br (g) – KBr(s) K(g) → K*(g) + e 1. endothermic 2. exothermic Br(g) + e Br (g) 2 Br2(g) → Br(g)