Question: During a reaction, some of the energy released by the system is used to move a mass up a hill, while the air temperature of the surroundings near the system increases by 50 K. What are the relative values for q, w and AU, respectively? A. q>0 ; w> 0;AU> 0 B. q> 0 ; w< 0 ; AU = 0 C. q< 0 ; w>0; AU = 0 D. q< 0 ; w< 0 ; AU < 0

Question: During a reaction, some of the energy released by the system is used to move a mass up a hill, while the air temperature of the surroundings near the system increases by 50 K. What are the relative values for q, w and AU, respectively? A. q>0 ; w> 0;AU> 0 B. q> 0 ; w< 0 ; AU = 0 C. q< 0 ; w>0; AU = 0 D. q< 0 ; w< 0 ; AU < 0

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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6. First aid kits often contain instant cold packs to treat sprains. These cold packs may contain ammonium nitrate and water. Ammonium nitrate dissociates in water as shown here: NH,NO, NH₂ (4) + NO₂ (a) You may find this information helpful Heats of Formation (AH,) NH4+ (aq) NO3 (24) NH,NO, Using your knowledge of thermochemistry, explain why ammonium nitrate is used. kJ/mol -132.8 -206.6 -365.6
Reaction 2 How much energy (in kJ) is released when 54,0 g of oxygen difluoride decomposes? Enter a positive number, Round to the nearest hundredth
7. Nitric oxide (nitrogen monoxide) gas can be oxidized in air to produce nitrogen pentoxide. Use Hess's Law to determine the enthalpy of reaction when this compound reacts as follows. Show all of your work. (T/I - 2) Target Equation: 2 N2(g) + 5 O2(g) 2 N₂O5(8) Use the following information: 1. N₂O5g) + H₂O(1) → 2 HNO3(1) AH = -77 kJ 2. 3. N2(g) + 3 O2(g) + H2(g) 2 HNO3(1) AH = -174 kJ 2 H₂(g) + O2(g) → 2 H₂O(1) AH = -572 kJ
H,A(aq) + BOH(aq)→ B,A(aq) + H,0(1) Assume that you have 0.4 grams of BOH (MW 40 g/mol) and excess H,A. AH=-802.3 kJ/mol is released when B,A is formed Assume that the reaction had an initial temperature of 23 C, what is the final temperature after the reaction goes to completion?) (Assume that the specific heat is 4.184 J/g*C) © 2015 Pearson Education, Inc.
What mass (in g) would an object need to have if travelling at 10.0 m/s caused it to possess a kinetic energy of 1.00 ? Select one: O a. 20.0 Ob. 10.0 O c 21.43 O d. 18.9 O e. 50.0
Pls help ASAP. Pls show all of your work and give ansewrs in significant figures. Pls write neatly and explain each step.
Part A Open the activity depicting Hess's Law. N:(g) + 0:(g) → 2NOg AH is an Extensive Property N: ( +0:(g) → NO(g) AH is an Extensive Property Click the button within the activity, and analyze the relationship between the two reactions that are displayed. The reaction that was on the screen when you started and its derivative demonstrate that the change in enthalpy for a reaction, AH, is an extensive property. Using this property, calculate the change in enthalpy for Reaction 2. AH Canges sign when a process is revTsed 2NO2) > N:(g) + 0: (g Reaction 1: C3 Hs(g)+ 502 (g)→3CO2 (g) + 4H2O(g), AH1 = -2043 kJ Hess's Law of Constant Heat Sumnation + N: (g) +0: (g) → deg Reaction 2: 5C3 Hs(g) +25O2(g)→15CO2(g) +20H,O(g), AH2 =? When two reactions are added together. the individual reaction enthalpies are summed. Notice that equal quantities of the same species, on both sides of the reaction arrow, cancel. NQg) +0: g) → NO: (g) Express your answer to four significant figures and include the…
How do we get the answers (in blue) to this question?
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
Using the AH values below for equations (7), (8) and (9), calculate an experimental AH for equation (10). Hint: use Hess's law. Note: These are NOT the values the experiment provides, so do not try to enter these on the Data Sheet. equation (7) Mg(s) + ½ 02(g) → MgO(s) AH = -602 kJ equation (8) MgO(s) +2HCI(aq) → MgCl2(aq) +H2O(1) AH = -136 kJ equation (9) Mg(s) + 2HCI(aq) → MgCl2(aq) + H2(g) AH = -452 kJ equation (10) H2(g) + ½ 02(g) → H2O(1) AH = ??? kJ
I Review | Constants | Periodic Table Open the activity depicting Hess's Law. N:(g) + 0: (g) → 2NOg) Part A AH is an Extensive Property + N: (g) + O:(g) → NO(g) AH is an Extensive Property Click the the screen when you started and its derivative demonstrate that the change in enthalpy for a reaction, AH, is an extensive property. Using this property, calculate the change in enthalpy for Reaction 2. AH Changes sign when a process is nevTNed 2NO2) N:(g) + 0:(g) button within the activity, and analyze the relationship between the two reactions that are displayed. The reaction that was on Hesss Law of Constant Heat Sunnaticn + N: (g) +0: (g) → dog Reaction 1: C3 Hs(g) + 502(g)→3CO2(g) + 4H20(g), AH1 = -2043 kJ When two reactions are added together, the individual reaction enthalpies are summed. Notice that equal quantities of the same species, on both sides of the reaction arnow, cancel. NQig) + +0: → NO: (2) Reaction 2: 5C3 Hs(g) + 2502(g)→15CO2 (g) + 20H2O(g), AH2 =? - N: (g) + O: (g) →…