Open the activity depicting Hess's Law.Part BN: (g) + 0: (g) →2NO(g)AH is an Extensive Property0:(g) NO(g)AH Changes sign when aClick on the process is reverseddisplayed. The reaction that was on the screen when you started and its derivative demonstrate that the reaction enthalpy, AH,changes sign when a process is reversed.button within the activity and analyze the relationship between the two reactions that areAH Canges sign when aprocess is revTied2NOg) N:(g) + O: (g)Hesss Law of ConstantHeat Sunation.+ N: (2) +0:(2)Consider the reactionWhen two reactions areadded together, theindividual reactionenthalpies are summed.Notice that equal quantitiesof the same species, on bothsides of the reaction arow,cancel.→ NO: (g)H2O(1)→H2O(g), AH = 44.0kJ+ N: (g) + O: (g) –→ NO: (g)What will AH be for the reaction if it is reversed?Express your answer with appropriate units.• View Available Hint(s)HA?ValueUnits Part AOpen the activity depicting Hess's Law.N:(g) + 0:(g) → 2NOgAH is an Extensive PropertyN: ( +0:(g) → NO(g)AH is an Extensive PropertyClick thebutton within the activity, and analyze the relationship between the two reactions that aredisplayed. The reaction that was on the screen when you started and its derivative demonstrate that the change in enthalpy for areaction, AH, is an extensive property. Using this property, calculate the change in enthalpy for Reaction 2.AH Canges sign when aprocess is revTsed2NO2)> N:(g) + 0: (gReaction 1: C3 Hs(g)+ 502 (g)→3CO2 (g) + 4H2O(g), AH1 = -2043 kJHess's Law of ConstantHeat Sumnation+ N: (g) +0: (g) → degReaction 2: 5C3 Hs(g) +25O2(g)→15CO2(g) +20H,O(g), AH2 =?When two reactions areadded together. theindividual reactionenthalpies are summed.Notice that equal quantitiesof the same species, on bothsides of the reaction arrow,cancel.NQg) +0: g) → NO: (g)Express your answer to four significant figures and include the appropriate units.N: (g) + O: (g) – → NO: (g)• View Available Hint(s)HA?AH2 =ValueUnits

Solve the questions using property of Hess's law and write value of ∆H for part A and B…

Open the activițty depicting Hess's Law. Part B N: (g)+ 0: (g 2NOg AH is an Extensive Property Np 0:(g NOg AH Changes sign when a Click on the process is reversed displayed. The reaction that was on the screen when you started and its derivative demonstrate that the reaction enthalpy. AH. changes sign when a process is reversed. button within the activity and analyze the relationship between the two reactions that are AH Changes sign when a proce is nried 2NO) Ni(g+ 0g) Hss Law of Costart Heat SuutioN Consider the reaction When two wactions are added together, the individal reaction enthalpies are summed. Notice that equal quantities of the same species, on both sides of the eaction anow, cancel NQg +0:g NO: H2O(1)→H2O(g), AH = 44.0kJ IN:i+O g → NO: What will AH be for the reaction if it is reversed? Express your answer with appropriate units. • View Available Hint(s) HA Value Units

Open the activițty depicting Hess's Law. Part B N: (g)+ 0: (g 2NOg AH is an Extensive Property Np 0:(g NOg AH Changes sign when a Click on the process is reversed displayed. The reaction that was on the screen when you started and its derivative demonstrate that the reaction enthalpy. AH. changes sign when a process is reversed. button within the activity and analyze the relationship between the two reactions that are AH Changes sign when a proce is nried 2NO) Ni(g+ 0g) Hss Law of Costart Heat SuutioN Consider the reaction When two wactions are added together, the individal reaction enthalpies are summed. Notice that equal quantities of the same species, on both sides of the eaction anow, cancel NQg +0:g NO: H2O(1)→H2O(g), AH = 44.0kJ IN:i+O g → NO: What will AH be for the reaction if it is reversed? Express your answer with appropriate units. • View Available Hint(s) HA Value Units

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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Instant cold packs used to ice athletic injuries on the field contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the endothermic reaction:NH4NO3(s) ---------> NH4 +(aq) + NO3 -(aq) In order to measure the enthalpy change for this reaction, 1.25 g of NH4NO3 is dissolved in enough water to make 25.0 mL of solution. The initial temperature is 25.8 °C, and the final temperature (after the solid dissolves) is 21.9 °C. Calculate the change in enthalpy for the reaction in kJ. (Use 1.0 g/mL as the density of the solution and4.18 J/g . °C as the specific heat capacity.)
< Question 21 of 29 O Attempt 2 When 0.376 g of sodium metal is added to an excess of hydrochloric acid, 3910 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) + 2 HCI(aq) 2 NaCl(aq) + H2(g) Enthalpy of reaction: 478.35 kJ Incorrect
СH;ОН (1) + Оz (в) — СО2 (s) + H,0 (1) ΔΗ. ræn = -1418 kJ mol How many grams of CO2 were produced if the reaction released 967 kJof heat?
Is the reaction exothermic or endothermic will any he be released or absorbed. If you said heat will be released or absorbed in the second part of the question calculate how much it will be released or absorbed round your answer to three significant digits. Please check your work
A chemist measures the energy change AH during the following reaction: Cl₂(g) + H₂(g) → 2 HC1 (g) AH=184. kJ Use the information to answer the following questions. endothermic. This reaction is... 0 exothermic. Suppose 28.0 g of Cl₂ react. Yes, absorbed. Yes, released. Will any heat be released or absorbed? No. 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. Round your answer to 3 significant digits. ☐kJ x10 X ?
A chemist measures the energy change AH during the following reaction: 2 NH;(g) - N(9)+3H,(9) AH=160, kJ Use the information to answer the following questions. O endothermic. This reaction is... O exothermic. Suppose 93.6 g of NH, react. O Yes, absorbed. O Yes, released. Will any heat be released or absorbed? O No. 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. Round your answer to 3 significant digits. Explanation Check 02021 McGraw Hill LLC. Al Rights Reserved Terms of Use Pivecy
3. During the experiment, when calculating AH using the formula AH=C x AT, can we calculate the AH without measuring the amount of water that we put inside the calorimeter? Explain why or why not. (max of 5 sentences) 4. You accidentally forgot to measure the mass of the octane that you transferred in the crucible. You already started the calorimeter and it is too late to stop the equipment. Is it still possible to calculate the energy (in Joules) of octane? Explain.(max of 2 sentences)
true or false? 3 The enthalpy changes for the reaction CO₂(g) + 3H₂(g) CH3OH(g) + H₂O(g) exceeds -52 kJ/mol.
Determine the amount of heat (in kJ) given off when 1.86 x 10° g of NO, are produced according to the equation: 2NO(g) + 0,(e) → 2NO.(e) AH = -114.6 kl/mol (N=14, 0=16) O 4.64 x 10' ky O 2.32 x 10' k O 2.32 x 10ʻ ki O 4.64 x 10' k) O 1.16 x 10' k
2. A student collect experimental results and show all calculation steps including units. Keep the correet significant figures. Part 1: Calculation of the calorimeter constant (15 pts) Mass of Mass of Temperature of cold water in calorimeter cold water hot water Temperature of hot water before mixing 57.3°C Final temperature of the water after mixing 36.8°C 61.0 g 56.2 g 22.6 °C Show calculations below. Part II: Conduct Reaction 1 between solutions of NaOH and HCI (20 pts) Volume of Volume of Density of the NaOH HCI Initial temperature of the solution in the calorimeter solution solution. solution 51.0 mL 52.0 mL 1.04 g/mL 22.6 °C Show calculations below. Final temperature of the reaction mixture 32.2 °C The calorimeter constant is: Enthalpy of the reaction, in kJ/mol, is
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.
Multiple Choice 1. When a match is lit, the air around the flame feels hot to the hand. Which statement best describes this observation? Heat is absorbed from the system, so it feels hotter. b. The reaction is endothermic. а. The potential energy of the match decreased. d. 3P6) + 10KCIO3 (5) → ЗРо + 10KCIO; (9) — с. 3P,O10 (9) + 10KCI + 9484 kJ 3P,O10 (6) AH = 3161 kJ/mol P е. (s) To answer questions 2 & 3, refer to the following information: A. synthesis reaction B. boiling a liquid C. subliming a solid D. dissolving a solute E. nuclear fission 2. Which of the following is always an example of an exothermic reaction? а. A d. D b. е. Е с. С 3. Which of the following would most likely have the smallest magnitude of enthalpy change? а. A d. B, C and D b. В е. А, В, С, D с. Е 4. How much energy is released when the temperature of 10.6 kg mass of a substance decreases by 15°C, if the substance has a specific heat of 1.6J/g°C? a. 0.10 kJ b. 0.25 kJ c. 0.51 kJ d. 1.0 x 10² kJ е. 250 k]