3. For which of the following statements is correct for the reaction 2NO2(g)→H2(g)+202(g)+66.4kJ A. exothermic, potential energy greater in reactants B. exothermic, potential energy greater in products C. endothermic, potential energy greater in products D. endothermic, potential energy less in reactants E. endothermic, potential energy less in products

3. For which of the following statements is correct for the reaction 2NO2(g)→H2(g)+202(g)+66.4kJ A. exothermic, potential energy greater in reactants B. exothermic, potential energy greater in products C. endothermic, potential energy greater in products D. endothermic, potential energy less in reactants E. endothermic, potential energy less in products

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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Part 2 The Haber process produces ammonia (NH3) for the chemical industry from nitrogen (N₂) and hydrogen (H₂) as shown in the chemical equation below. This is a reversible reaction. N2 (8) + 3H2(g) → 2NH3 (8) AH = -92 kJ mol-¹ (exothermic) The following questions relate to the effect of changing factors that influence the direction of the above reaction, according to Le Chatelier's principle. For each change in factor (i - iv) listed in the Table, you need to: state the direction of equilibrium, give a reason for your choice, identify if the amount of ammonia produced will increase or decrease. Factor Decrease in concentration of N₂ i) ii) Increase in pressure iii) Increase in temperature iv) A catalyst is added Direction (shift) of equilibrium Scientific explanation for stated direction of equilibrium. Amount of NH3 Increases / decreases Part 3 During this reaction, compromises are made to speed up and maximise the production of ammonia. i) ii) Suggest why a moderate amount of…
does adding temperature to a chemical reaction favor the reaction endothermically?
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7. Which of the following technologies are considered non-renewable energy sources? Choose ALL that apply. a. Coal Power Plants b. C. Hydrogen Fuel Cells Fossil Fuel Power Plants a. b. C. 8. Which of the following reactions are endothermic? Choose ALL that apply. H2(g) + 1/2O2(g) H₂O(g); AH = -243 kJ/mol ¹1/2N2(g) + ¹//202(g) + 90.7 kJ → NO(g) CO(g) + 111 kJ C(s) + ¹1/202(g) d. Hydroelectric Generators Solar Panels e. f. Wind Turbines a. Acid lonization Constant (K₂) b. Base lonization Constant (K) C. Equilibrium Constant (Keg) d. e. f. HI(g)→→ ¹1/₂2H2(g) + ½l2(g); AH = −26 kJ/mol H₂O(g) · H2(g) + ½O2(g); AH = +243 kJ/mol + O2(g) 2NO N2(g) + 181.4 kJ (g) 9. Which equilibrium constant would be most relevant to the following system in equilibrium: HC₂H3O2(aq) → H*( (aq) + C₂H3O₂ (aq) Partial Pressure Equilibrium Constant (K₁) d. e. Solubility Product Constant (Ksp) f. Water lon Product Constant (Kw)
4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
Name the alkenes below. Use ONLY E/Z designators to indicate stereochemistry. H3C H Ja H CH₂-C H CH3 CH₂CH3
a. How much energy is required to decompose 850 g of PCl3, according to the reaction below? The molar mass of PCl3 is 137.32 g/mol and may be useful.4 PCl3(g) → P4(s) + 6 Cl2(g) ΔH°rxn = +1207 kJ b. The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to raise the temperature of 6.00 g of water from 22.0°C to 57.0°C? 1.99 × 10-2 J 1.98 × 103 J 65.0 J 50.2 J 878 J
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
Consider the reaction. 2Fe2O3⟶4Fe+3O2 Δ?∘rxn=+824.2 kJ The decomposition of 74.0 g of Fe2O3 results in A.) the release of 382 kJ of heat. B.) the absorption of 191 kJ of heat. C.) the release of 191 kJ of heat. D.) the absorption of 30500 kJ of heat. E.) the release of 30500 kJ of heat. F.) the absorption of 382 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.
Assignments View Available Hint(s) HA mass of the steel = Value Units 90 12:51 acer
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