3. For the following reactions, Identify the unknown, the ?, and circle the change for each of the energy systems. Changes in the Strong Energy Interaction are determined by the net amount of bounds broken or formed and changes in the Electric Energy are determined by the separation of like charges. i. 6429Cu → 6428NI + ? + V a. The unknown "?" is b. PEelectric: increases, decreases, no change c. PEstrong: increases, decreases, no change d. Energy: Exothermic e. Mass: increases, decreases, no change ii. 189F + ? → 180 + v a. The unknown "?" is b. PEelectric: increases, decreases, no change c. PEstrong: increases, decreases, no change d. Energy: Exothermic e. Mass: increases, decreases, no change

3. For the following reactions, Identify the unknown, the ?, and circle the change for each of the energy systems. Changes in the Strong Energy Interaction are determined by the net amount of bounds broken or formed and changes in the Electric Energy are determined by the separation of like charges. i. 6429Cu → 6428NI + ? + V a. The unknown "?" is b. PEelectric: increases, decreases, no change c. PEstrong: increases, decreases, no change d. Energy: Exothermic e. Mass: increases, decreases, no change ii. 189F + ? → 180 + v a. The unknown "?" is b. PEelectric: increases, decreases, no change c. PEstrong: increases, decreases, no change d. Energy: Exothermic e. Mass: increases, decreases, no change

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

Experimental observations of a biochemical reaction have indicated that the reaction releases free energy to its surroundings. What is the name for this type of reaction and what sign is associated with its value for change of free energy? a. Exothermic, negative b. Exothermic, positive c. Endothermic, negative d. Exergonic, negative e. Endothermic, positive
Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change An exothermic chemical reaction between a solid and a liquid results in gaseous products. A solid precipitates from a solution, absorbing heat as it does so. A gas expands, absorbing heat from its surroundings. Is this change spontaneous? Yes. No. Can't decide with information given. Yes. No. O Can't decide with information given. Yes. No. Can't decide with information given. X
Values for Kp and Kc remain the same regardless of how the reaction is written. a. True b. False In a heating curve, an increase in kinetic energy occurs during a phase change. a. True b. False
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
Determine whether each of the following reactions would have a positive or negative AS value. a. 4BrCl (g) + C (s) → CCl4 (g) + 2Br2 (1) b. CS2 (g) + 2HCl (g) → CSC1₂ (g) + H₂S (g) c. SF4 (g) + 2H₂O(g) d. 2Al(s) + 2NaOH (aq) + 2H₂O (1) SO₂ (g) + 4HF (g) ->>> 2NaAlO2 (s) + 3H₂ (g)
Classify each of the statements as true or false. False Truc An exothermic reaction is always spontaneous. The entropy ofa substance increases when a solid melts into a liquid at any temperature. Product formation is never favored in a reaction with a negative AH and a positive AS. For an endothermic reaction, a decrease in temperature results in a decrease in the equilibrium constant. A reaction will have an equilibrium constant that is less than one if AG" for the reaction is positive. Entropy increases as the temperature decreases. Answer Bank 2°C Mostly cloudy A a ENG 01/0
Which one of the following processes requires the most energy? O Be2*(g) → Be3+(g) + e- O C(g) → C*(g) +e- O B2*(g) B3+(g) + e- Oc2+(g) C3+(g) + e- O Be*(g) Be2*(g) + e- ->
Use thermochemical data given in the table to decide whether the equilibrium constant for each of the following reactions will increase or decrease with temperature. Substance AH; (kJ/mol) CO(g) CO₂ (g) CS₂(g) CH₁ (9) H₂(g) H₂S(g) H₂O(g) N₂ (9) NH3 (9) O₂(g) -111 -394 117 -74.9 0 -20.5 -242 0 -45.9 0 a. CO₂(g) + H₂(g) → CO(g) + H₂O(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase. b. 2CO2 (g) 2CO(g) + O2(g) O The equilibrium constant will increase with temperature increase. O The equilibrium constant will decrease with temperature increase.
→ C ||| = www-awa.aleks.com/alekscgi/x/Isl.exe/1o_u-lgNslkr7j8P3jH-lvgXwPgmUhvlCeeBZbuluBY TUHz/m/I OTHERMOCHEMISTRY Calculating the heat of reaction from molar reaction enthalpy a... A chemist measures the energy change AH during the following reaction: Cl₂(g)+H₂(g) → 2 HCl(g) Use the information to answer the following questions. This reaction is... Suppose 68.3 g of Cl₂ react. Will any heat be released or absorbed? 75°F Sunny If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Explanation ΔΗ = - 184. kJ Round your answer to 3 significant digits. Check endothermic. O exothermic. O Yes, absorbed. O Yes, released. O No. H Q Search 0 0x10 X S a C 4 4 1/3 Andrew V Relate © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 25 4 ? ➤III olo Ar 7:37 PM 7/16/2023
1.) Complete A and B to move on. a.) Write the complete, balanced chemical equation for the following reaction on a separate sheet of paper. Provide products where they are not given. Assume that the reaction is spontaneous. Propane (C3H8) + oxygen → carbon dioxide + water Type the sum of the coefficients in the equation into the answer blank. If there is no coefficient, count it as one. Include ( g, s, l, or aq) b.) Write the complete, balanced chemical equation for the following reaction on a separate sheet of paper. Provide products where they are not given. Assume that the reaction is spontaneous. Diphosphorus pentoxide + water → Type in the coefficient and formula for the product in the equation that contains phosphorus. Include ( g, s, l, or aq)
At -5.92 °C the pressure equilibrium constant K = 5.9 for a certain reaction. P Here are some facts about the reaction: • If the reaction is run at constant pressure, 127. kJ/mol of heat are released. • The constant pressure molar heat capacity C • The net change in moles of gases is -1. = 2.41 J mol -1. K¹. -1 р Yes. ☐ x10 Using these facts, can you calculate K at -27. °C? ○ No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Р If you said no, can you at least decide whether K at -27. °C will be bigger or smaller than K, at −5.92 °C? П Yes, and K, will be р bigger. Yes, and K smaller. will be No. ☑
Consider the reaction. vopica! Submit Answe Use the References to access important values if needed for this question. 2SO₂(g) + O₂(g) 2503(g) Using the standard thermodynamic data in the tables linked above, calculate AGxn for this reaction at 298.15K if the pressure of each gas is 11.74 mm Hg. ANSWER: kj/mol Retry Entire Group 2 more group attempts remaining