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1. Show your work for all calculations. When 1.104 grams of iron metal are mixed with 26.023 grams of hydrochloric acid in a coffee cup calorimeter, the temperature rises from 25.2 °C to a maximum of 33.5 °C. The reaction that occurs is given below 2 Fe(s) +6 HC1(aq) → 2 FeCL(aq) + 3 H, (g) (1 • Determine the amount of heat (in J) absorbed by the reaction mixture. Assume that the specific heat capacity of the mixture same as the specific heat capacity of water. How much heat (in Duac mleace

1. Show your work for all calculations. When 1.104 grams of iron metal are mixed with 26.023 grams of hydrochloric acid in a coffee cup calorimeter, the temperature rises from 25.2 °C to a maximum of 33.5 °C. The reaction that occurs is given below 2 Fe(s) +6 HC1(aq) → 2 FeCL(aq) + 3 H, (g) (1 • Determine the amount of heat (in J) absorbed by the reaction mixture. Assume that the specific heat capacity of the mixture same as the specific heat capacity of water. How much heat (in Duac mleace

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Pre-laboratory Assignment: Calorimetry and Hess’s Law

Note that the thermometer must be clamped in place using the slotted stopper and utility clamp/stand. You may also want to place the nested cups in a medium beaker for extra stability. Pre-laboratory Assignment: Calorimetry and Hess's Law 1. Show your work for all calculations. When 1.104 grams of iron metal are mixed with 26.023 grams of hydrochloric acid in a coffee cup calorimeter, the temperature rises from 25.2 °C to a maximum of 33.5 °C. The reaction that occurs is given below. 2 Fe(s) +6 HCl(aq) → 2 FeCL,(aq) + 3 H, (g) (12.12) • Determine the amount of heat (in J) absorbed by the reaction mixture. Assume that the specific heat capacity of the mixture is the same as the specific heat capacity of water. • How much heat (in J) was released by the reaction that occurred? • Is this reaction exothermic or endothermic? Is AH reaction positive or negative? • Under constant pressure conditions (as used in this experiment), the heat released by the reaction equals the reaction enthalpy, Greleased=AHrenction. Determine AHreaction in Joules per gram of metal used (J/g). • Determine AHreaction in kilojoules per mole of metal used (kJ/mol). • Determine AHreaction in kilojoules for the balanced reaction equation provided (kJ). 2. Consider the following three reactions: 2 Fe(s) +6 HC1(aq) → 2 FeCL (aq) +3 H, (g) Fe,0,(s)+6 HCl(aq) 2 FeCl, (aq) +3 H,O(1) AHA (12.13) - AHB (12.14) 2 H, (g) + 0,(g) –→ 2 H,O(1) 12.15) Show how these equations must be summed together according to Hess's Law to determine AH for the combustion of iron (target equation shown below). Also show clearly how the AH values of each of the three reactions must be manipulated to determine the enthalpy of combustion of iron. 4 Fe(s) +30,(g)→ 2 Fe,O, (s) 3. Using tabulated AH values in the text, determine the enthalpy change (in kJ) that occurs during the formation of water from its AH-? (12.16) elements: 2 H, (g) + 0, (g) - 2 H,O(1) (12.17) AH=? Note that this value (and the equation) will be used in your data analysis for this lab.
Transcribed Image Text:Note that the thermometer must be clamped in place using the slotted stopper and utility clamp/stand. You may also want to place the nested cups in a medium beaker for extra stability. Pre-laboratory Assignment: Calorimetry and Hess's Law 1. Show your work for all calculations. When 1.104 grams of iron metal are mixed with 26.023 grams of hydrochloric acid in a coffee cup calorimeter, the temperature rises from 25.2 °C to a maximum of 33.5 °C. The reaction that occurs is given below. 2 Fe(s) +6 HCl(aq) → 2 FeCL,(aq) + 3 H, (g) (12.12) • Determine the amount of heat (in J) absorbed by the reaction mixture. Assume that the specific heat capacity of the mixture is the same as the specific heat capacity of water. • How much heat (in J) was released by the reaction that occurred? • Is this reaction exothermic or endothermic? Is AH reaction positive or negative? • Under constant pressure conditions (as used in this experiment), the heat released by the reaction equals the reaction enthalpy, Greleased=AHrenction. Determine AHreaction in Joules per gram of metal used (J/g). • Determine AHreaction in kilojoules per mole of metal used (kJ/mol). • Determine AHreaction in kilojoules for the balanced reaction equation provided (kJ). 2. Consider the following three reactions: 2 Fe(s) +6 HC1(aq) → 2 FeCL (aq) +3 H, (g) Fe,0,(s)+6 HCl(aq) 2 FeCl, (aq) +3 H,O(1) AHA (12.13) - AHB (12.14) 2 H, (g) + 0,(g) –→ 2 H,O(1) 12.15) Show how these equations must be summed together according to Hess's Law to determine AH for the combustion of iron (target equation shown below). Also show clearly how the AH values of each of the three reactions must be manipulated to determine the enthalpy of combustion of iron. 4 Fe(s) +30,(g)→ 2 Fe,O, (s) 3. Using tabulated AH values in the text, determine the enthalpy change (in kJ) that occurs during the formation of water from its AH-? (12.16) elements: 2 H, (g) + 0, (g) - 2 H,O(1) (12.17) AH=? Note that this value (and the equation) will be used in your data analysis for this lab.
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