Decide how the sketches below would be listed, if they were listed in order of decreasing potential energy. That is, select "1" beside the sketch that shows the system with the highest potential energy, select "2" beside the sketch that shows the system with the next highest potential energy, and so on. Note for advanced students: since the units of each charge are not written, you may assume any convenient and reasonable unit, for example coulombs or multiples of e. +2 O 1 (highest) 02 0 3 O4 (lowest) O 1 (highest) 02 0 3 04 (lowest) ✪ 1 +3 O 1 (highest) 02 0 3 O 4 (lowest) O 1 (highest) 02 0 3 O4 (lowest)

Decide how the sketches below would be listed, if they were listed in order of decreasing potential energy. That is, select "1" beside the sketch that shows the system with the highest potential energy, select "2" beside the sketch that shows the system with the next highest potential energy, and so on. Note for advanced students: since the units of each charge are not written, you may assume any convenient and reasonable unit, for example coulombs or multiples of e. +2 O 1 (highest) 02 0 3 O4 (lowest) O 1 (highest) 02 0 3 04 (lowest) ✪ 1 +3 O 1 (highest) 02 0 3 O 4 (lowest) O 1 (highest) 02 0 3 O4 (lowest)

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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nuraipy changes in chemical reactions Read through pages 18-20 in your laboratory manual for information on how to calculate the enthalpy change in a solution. Part A - Calculating ms In a calorimetry experiment 5.6 g of potassium hydroxide is dissolved in 400 mL water in a thermos flask. The temperature increase in the solution is 7 °C. The effective mass of the glass in the thermos flask (mcal) is 0.040 kg. The heat capacity of the solution (Cs) is 4.04 kJkg-¹K-1¹. The heat capacity of the calorimeter (Ccal) is 0.387 kJkg-¹K-1. Remember to enter your answer using the specified number of significant figures, but keep the entire number in your calculator for use in further calculations. Calculate the total mass of solution in kilograms (ms) Give your answer to four significant figures. ▾ View Available Hint(s) Hint 1. Calculating ms mg = mass water (kg) + mass solute (kg) —| ΑΣΦ Submit Request Answer ? kg < Pear 10
A scientist measures the standard enthalpy change for the following reaction to be 6.7 kJ : CO(g) + H,O(1)–CO;{g) + H2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO(g) is kJ/mol.
(incorrect) Calculate the standard enthalpy of reaction for the following reaction using the appropriate standard enthalpies of formation AH [SiCl4 (g)] = -657.0 kJ/mol; Other relevant thermodynamic quantities can be found in the appendix at the end of the textbook. SiO₂ (s) + 4 HCI (g) → SiCl4 (g) + 2 H₂O(g) -104.2 kJ 104.2 kJ -137.2 kJ -139.3 kJ (Your answer) 139.3 kJ (Correct answer)
Unit Name: Thermodynamic Chemistry investigate and analyse energy changes and rates of reaction in physical and chemical processes, and solve related problems; Calculate the enthalpy of the following reaction:
5. When 1.00g of NaCl (MM 58.44 g/mol) is dissolved in 50.00g of water, the temperature drops by 0.319°C. This temperature change is only detectable by the most sensitive thermometers. If this process takes place in a very well insulated calorimeter, no calorimeter constant is needed. a. Calculate the enthalpy change per gram of NaCl. b. Calculate the enthalpy change per mole of NaCl.
CHAPTER 5 - PRINCIPLES OF CHEMICAL REACTIVITY: EN Previous Page 3 of 5 endothermic ✓ exothermic When 1 mole of I2 (g) reacts with Cl₂ (g) to form ICI(g) according to the following equation, 26.8 kJ of energy are evolved. 1₂ (9) + Cl₂ (9) → 21C1(g) What is the value of q? kJ NOV 11 Next → othermic or exothermic? #tv ♫ P 100 Use the References to access DO Cengage Learning | C MacB
Given these reactions, where X represents a generic metal or metalloid 1) H, (g) + 0,(g) → H,0(g) AH1 = -241.8 kJ 2) X(s) + 2 Cl,(g) → XCl,(s) AH2 = +475.9 kJ 3) H,(g) + CL,(g) HCl(g) АНз 3 —92.3 kJ → 4) X(s) + O,(g) –→ XO,(s) AH4 = -748.7 kJ 5) Н, О(2) — н,00) AH5 = -44.0 kJ what is the enthalpy, AH, for this reaction? XCI, (8) + 2H,О() — ХО,(8) + 4 HCI(g)
A chemist measures the enthalpy change AH during the following reaction: 2 H,O(1) + O2(9)→2 H,O2(1) ДН-196. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ x10 4H, 0, (1) → 4H,0(1) + 20, (g) kJ 2H,0, (1) → 2H,0(1) + 0, (g) I kJ 1 H,0(1) + 0,(2) - H,0,) H,0, (1) O kJ
How much energy is required to break the bonds in the molecule of NO, BCl3, and NO2? and How do I find the ΔH of the molecule from the elements in their standard states?
Use your results from #4 and data Table 8.1 to calculate the value of DHf for Mg†² (aq) Note: You must write out the formation equations of all products and reactants and sum to find the change in enthalpy for the formation of the cation (like example 8.3). Failure to do so will result in zero credit.
The first step in the production of nitric acid from ammonia involves the oxidation of NH3. 4 NH3(g) + 5 O₂ (g) → 4 NO(g) + 6 H₂O(g) 2 a Use standard enthalpies of formation from the table below to calculate the standard enthalpy change for this reaction. Species AfH (kJ/mol) NH3(g) -45.90 NO(g) +90.29 H₂O(g) -241.83 Standard enthalpy change Submit = kJ/mol-rxn
thermometer A 59.2 g sample of iron is put into a calorimeter (see sketch at right) that contains 200.0 g of water. The iron sample starts off at 95.8 °C and the temperature of the water starts off at 24.0 °C. When the temperature of the water stops changing it's 27.1 °C. insulated container The pressure remains constant at 1 atm. water Calculate the specific heat capacity of iron according to this experiment. Be sure your answer is rounded to 2 significant digits. sample a calorimeter g.°C Explanation Check O2021 McGraw-Hill Education. All Rights Reserved Terms of Usse Privacy Accessibi MacBook Ai