Using any resources available to you (e.g., textbook, CRC Handbook, online sources), obtain and use standard heats of formation and Hess' Law to calculate the standard heat of reaction AH° for the decomposition of H₂O2. Show ALL your work below, starting with the balanced equation, and summarize your results in the table provided. NOTE: Do NOT simply look up the value of AH for this reaction and write it below - you NEED to use standard heat of formation, show your work, etc. Heat of Formation for H₂O₂(aq) (kJ/mol) Heat of Formation for H₂O(1) (kJ/mol) Heat of Formation for O₂(g) (kJ/mol) Calculated AHpn (J/mol)

Using any resources available to you (e.g., textbook, CRC Handbook, online sources), obtain and use standard heats of formation and Hess' Law to calculate the standard heat of reaction AH° for the decomposition of H₂O2. Show ALL your work below, starting with the balanced equation, and summarize your results in the table provided. NOTE: Do NOT simply look up the value of AH for this reaction and write it below - you NEED to use standard heat of formation, show your work, etc. Heat of Formation for H₂O₂(aq) (kJ/mol) Heat of Formation for H₂O(1) (kJ/mol) Heat of Formation for O₂(g) (kJ/mol) Calculated AHpn (J/mol)

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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F When Fe₂O3(s) reacts with H₂(g) to form Fe(s) and H₂O(g), 98.8 kJ of energy are absorbed for each mole of Fe₂O3(s) that reacts. Write a balanced thermochemical equation for the reaction with an energy term in kj as part of the equation. Note that the answer box for the energy term is case sensitive. Use the SMALLEST INTEGER coefficients possible and put the energy term in the last box on the appropriate side of the equation. If a box is not needed, leave it blank. 20 Submit Answer 4 R F F4 V + % 5 [Review Topics] [References] Use the References to access important values if needed for this question. Retry Entire Group T G ♫ TV STA © B + MacBook Air FG 6 A Y H 7 more group attempts remaining & 7 N U J * 8 00 - M DII I K ( 9 V H s DD F9 O + O P F10 P A + command option Previous F11 { = Next> Save and Exit 40) F12 A delete S retur
5575082893418928809969212&elSBN=9781305657571&... Tp Q Search this co References Use the References to access important values if needed for this question. A student determines the heat of dissolution of solid cobalt(II) chloride using a coffee-cup calorimeter of negligible heat capacity. When 1.58 g of CoCl,(s) is dissolved in 101.00 g of water, the temperature of the solution increases from 25.00 to 27.42 °C. Based on the student's observation, calculate the enthalpy of dissolution of CoCl,(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. AH dissolution kJ/mol Submit Answer
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Themeter Mod Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 92.55 grams of zinc to 97.73 °C and then drops it into a cup containing 78.30 grams of water at 21.37 °C. She measures the final temperature to be 28.88 °C. Using the accepted value for the specific heat of zinc (See the References tool), calculate the calorimeter constant. Calorimeter Constant = 3/°C Submit Answer Retry Entire Group 8 more group attempts remaining
When N₂(g) reacts with H₂(g) to form NH3(g), 92.2 kJ of energy are evolved for each mole of N₂(g) that reacts. Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation. Note that the answer box for the energy term is case sensitive. Use the SMALLEST INTEGER coefficients possible and put the energy term (including the units) in the last box on the appropriate side of the equation. If a box is not needed, leave it blank. + + +
Write balanced equations that describe the formation of thefollowing compounds from elements in their standard states,and then look up the standard enthalpy of formation foreach substance in Appendix C: (a) H2O2(g), (b) CaCO3(s),(c) POCl3(l), (d) C2H5OH(l).
In the recovery of iron from iron ore, the reduction of the ore is actually accomplished by reactions involving carbon monoxide. Use the following thermochemical equations, Fe,O3(s) + 3CO(g) 2Fe(s) + 3CO,(g) AH° = - 28 kJ 3Fc,O3() + CO(g) 2Fe3O4() + CO,(g) AH = -59 kJ FezO4(s) + CO(g) 3FcO(s) + CO,(g) AH° = +38 kJ to calculate AH° for the reaction FeO() + CO(g) Fe(s) + CO2(g) AH° = i kJ
Calculating a Heat of Formation Using Hess’s LawAs discussed in lecture, the simplest and most general method for determining theenergy change during a chemical reaction involves the use of the heat of formation (ΔHf) for thereactants and products. Conceptually, the heat of formation is the heat released or absorbedwhen one mole of the substance is created from its elements at standard temperature andpressure. In some cases, this number can be measured directly (i.e. by reacting the elements at1.0 atm and 25oC and observing the heat given off). In most cases, however, this is notpractical. For instance, the direct calculation of the ΔHf for magnesium oxide would involveburning magnesium metal in a pure oxygen atmosphere; while such a reaction is certainlypossible, it would difficult to measure changes in temperature since the reaction is highlyexothermic and the product is a solid powder. Instead, in this lab you will be calculating the ΔHf for magnesium oxide by determiningthe heat of…
Johnson and Steele determined the standard enthalpy of combustion of UO₂(s) in gaseous fluorine. The products of combustion are UF(s) and O2(g). The measured value of the enthalpy of combustion is -1112.6 kJ mol-¹ (per mole of UO₂), and the standard enthalpy of formation of UF(s) is -2197.7 kJ mol-¹. Calculate the standard enthalpy of formation of UO2(s) in kJ mol-¹.
Calculate the standard enthalpy change for the reaction 2A +B= 2C+2D Use the following data: AH; (kJ/mol) Substance A -225 В -375 C 199 D -475 Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HÀ ? kJ ΔΗ Value mol
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 90.62 grams of zinc to 97.68 °C and then drops it into a cup containing 84.45 grams of water at 23.94 °C. She measures the final temperature to be 30.58 °C. Using the accepted value for the specific heat of zinc (See the References tool), calculate the calorimeter constant. Calorimeter Constant J/°C.
50.00 mL of 1.0 M NaOH solution at 18.0°C is mixed with 50.00 mL of 1.0 M HCI solution also at 18.00°C in a calorimeter. The mixture was allowed to react to completion and the temperature of the mixture rose to 23.60°C. Use the following information to calculate the enthalpy of the reaction. Density of the mixture is 1. lg/mL Specific heat capacity of mixture 4.18J/gK Heat capacity of calorimeter 8.65J/K (Note: Express your answer to two significant figures and do no include unit (KJ/mol) in the calculated answer).
[Review Topics] [Ref Calculate the standard enthalpy change, AH°, for the following reaction at 25°C. Fe2O3 (s) + 2A1(s) → 2Fe(s) + Al, O3 (s) What is the enthalpy change per mole of iron? Substance AH, kJ/mol Fe,O3 (s) -825.5 -1675.7 Standard enthalpy change = kJ Enthalpy change per mole of iron = Submit Answer Retry Entire Group 9 more group attempts remaining LAON tv P.