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 +2 O 1 (highest) 2 3 4 (lowest) O 1 (highest) 2 3 4 (lowest) +5 X O 1 (highest) 2 0 3 ○ 4 (lowest) O 1 (highest) 2 3 ○ 4 (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 +2 O 1 (highest) 2 3 4 (lowest) O 1 (highest) 2 3 4 (lowest) +5 X O 1 (highest) 2 0 3 ○ 4 (lowest) O 1 (highest) 2 3 ○ 4 (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...

See similar textbooks

Similar questions

4. Hess's Law Calculate AH for the reaction: 2 C(s) + H2(g) → C:H2(g), given the following chemical equations and their respective enthalpy changes: C2H2(g)+02(g)→2CO2(g)+H20(1) AH, = -1299.6 kJ (1) %3D C(s)+02(g)→CO2(g) AH, = -393.5 kJ (2) H2(g)+502(g)→H20(1) AH3 = -285.8 kJ (3)
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
Determine the enthalpy of the reaction: 3Fe,O; (s) + CO (g) → CO, (g) + 2Fe;O4 (s), given the following reactions. 38. Fe,O3 (s) + 3CO (g) → 2Fe (s) + 3CO, (g) AH= -28.0 kJ 3Fe (s) + 4CO2 (s) → 4CO (g) + Fe;O4 (s) AH =+12.5 kJ A) 40.5 +109 -59.0 -109
Given the following reactions Reactions Enthalpies of Reaction 1 Na(s) + Cl2(8) → Na(g) + Cl(g) AH = 257 kJ 2 Na(g) + Cl(g) → Na*(g) + Cl(g) AH = 164 kJ 1 Cl2(g) → Nacl(s) Na(s) + AH = -333 kJ Use Hess' Law to determine the AH for the following reaction: (watch your states and charges) Na*(g) + Cl'(g) → NaCI(s) X kJ
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
When 3.8 g A are reacted with 8.5 g D, according to the balanced chemical equation below, 33 kJ of energy are released. Please calculate the enthalpy for this reaction when 3 moles of G are produced. 2A + 3D = 2Z + 3G given molar masses: A = 141.8 g/mole D = 63.996 g/ mole Z = 4.032 g/ mole G = 56.028 g/ mole
2. a. Determine the standard heat of formation, AH for the following reaction using the Data from the Table. C3H12 ) + 802(g) → 5CO2 + 6H₂O b. State whether the reaction is exothermic or endothermic. Explain. c. Rewrite the equation as thermochemical equations in two different ways to include the heat calculated in (2a). d. Draw a detail Energy Diagram representing the thermochemical equation in Ⓒ illustrating the the reactants and products and their positions.
A model for the compound 2,2- dimethylbutane is shown. Write a balanced chemical equation that shows the formation of 2,2-dimethylbutane from the elements carbon (C) and hydrogen). (Use the smallest integer coefficients possible and do not include states.) A model for the compound 2,2-dimethylbutane is shown Write a balanced chemical equation that shows the formation of 2,2-dimethylbutane from the elements carbon (C) and hydrogen (H₂) (Use the smallest integer coefficients possible ond do not include states.)
A chemist measures the enthalpy change AH during the following reaction: COCL,(9) + 4 NH,(g)–+cO(NH,),(s) + 2 NH,Cl(s) AH=-559. kJ Use this information to complete the table below. Round each of your answers to the neare reaction AH co(NH,),(-) + NH,CI(3) - coC, () + 2NH, (2) 3coCI, (3) + 12NH, (3) - 3c0(NH,), (-) + 6NH,CI(s) co(NH,),() + 2NH,C1(«) → COCI, (3) + 4NH, (2) Explanation Check MacBook Air 20 F1 F3 F4 F5 F6 F @ & くC
Use the molar bond enthalpy data in the table to estimate the value of AHin for the equation. rxn NH3(g) + 2O₂(g) → HNO3(g) + H₂O(g) The bonding in the molecules is shown. H AHixn = H O اس ای H + Bond O-H 0-0 C-O 0=0 C=O C-C C=C C=C C-H C-F C-Cl C-Br C-N C=N kJ. mol-¹ 464 142 351 502 730 347 615 811 414 439 331 276 293 615 Bond C=N N-H N-O N=N N=O F-F Cl-Cl Br-Br H-H H-F H-Cl H-Br H-S S-S kJ · mol-¹ 890 390 201 418 607 155 243 192 435 565 431 368 364 225 kJ.mol-¹
Consider the following reaction whose enthalpy change Is ΔΗ- w S(s) + H,(g) -> H,S(g) AH = w This equation is obtained using the following equations along with the Hess law H,(g) + %0,(g) -> H,0() AH = x S(s) + 0,(g) > So(g) AH = y ΔΗ Υ H,S(g) + 1%0,(g) -> H,O() + SO,(g) AH = z What is the relationship between enthalples w, x, y and z? O a. w=z+y -x O b. w=x + y -z O. W=S-Xx -y O d. w=x -y -z O e. w=z-y -x Clear my choice