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ADVANCED STUDY ASSIGNMENT 1. 0.500 g of Ca is added to 50.0 mL of 1.0 M HCI. Once reaction is complete, the temperature of the solution has risen from 25.2 °C to 71.4 °C. The reaction proceeds by the following equation: Cа (8) + 2 H'(аq) — Са"(аq) + H(g) Calculate the heat gained by the solution q= mos•AT, where s = 4.184 J/g•°C m = mass in grams s- specific heat in J/g• °C AT = final temp. - initial temp. Fsoln = oin= kJ b. Heat lost by the reaction: q.xn = -quoln kJ AH kJ/mol Ca Calculate the heat of reaction:

ADVANCED STUDY ASSIGNMENT 1. 0.500 g of Ca is added to 50.0 mL of 1.0 M HCI. Once reaction is complete, the temperature of the solution has risen from 25.2 °C to 71.4 °C. The reaction proceeds by the following equation: Cа (8) + 2 H'(аq) — Са"(аq) + H(g) Calculate the heat gained by the solution q= mos•AT, where s = 4.184 J/g•°C m = mass in grams s- specific heat in J/g• °C AT = final temp. - initial temp. Fsoln = oin= kJ b. Heat lost by the reaction: q.xn = -quoln kJ AH kJ/mol Ca Calculate the heat of reaction:

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
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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l T-Mobile Wi-Fi ? 2:23 PM @ O 65% Exp 10B Second Lab.pdf 5 of 5 Experiment 52 Name Section ADVANCED STUDY ASSIGNMENT 1. 0.500 g of Ca is added to 50.0 mL of 1.0 M HCI. Once reaction is complete, the temperature of the solution has risen from 25.2 °C to 71.4 °C. The reaction proceeds by the following equation: Са (s) + 2 H'(аq) —> Са" (аq) + H(g) Calculate the heat gained by the solution q = m•s•AT, where s = 4.184 J/%•°C m = mass in grams s = specific heat in J/g• °C AT = final temp. - initial temp. a. 9soln = soin = kJ kJ b. Heat lost by the reaction: q;xn = -qsoln Calculate the heat of reaction: AH° = kJ/mol Ca c. 2. Using Hess' Law, calculate the enthalpy of formation for C,Hg (g) using the following thermodynamic data. C(s) + O2(g) → CO2(g) AH° =-393.5 kJ/mol H2(g) + ½O(g) → H,O(1) AH° = -285.8 kJ/mol C3Hs(g) + 502(g) → 3CO2(g) + 4H;O(1) AH° = =2199.0 kJ/mol 277
Transcribed Image Text:l T-Mobile Wi-Fi ? 2:23 PM @ O 65% Exp 10B Second Lab.pdf 5 of 5 Experiment 52 Name Section ADVANCED STUDY ASSIGNMENT 1. 0.500 g of Ca is added to 50.0 mL of 1.0 M HCI. Once reaction is complete, the temperature of the solution has risen from 25.2 °C to 71.4 °C. The reaction proceeds by the following equation: Са (s) + 2 H'(аq) —> Са" (аq) + H(g) Calculate the heat gained by the solution q = m•s•AT, where s = 4.184 J/%•°C m = mass in grams s = specific heat in J/g• °C AT = final temp. - initial temp. a. 9soln = soin = kJ kJ b. Heat lost by the reaction: q;xn = -qsoln Calculate the heat of reaction: AH° = kJ/mol Ca c. 2. Using Hess' Law, calculate the enthalpy of formation for C,Hg (g) using the following thermodynamic data. C(s) + O2(g) → CO2(g) AH° =-393.5 kJ/mol H2(g) + ½O(g) → H,O(1) AH° = -285.8 kJ/mol C3Hs(g) + 502(g) → 3CO2(g) + 4H;O(1) AH° = =2199.0 kJ/mol 277
.ll T-Mobile Wi-Fi ? 2:23 PM @ O 66% f Data - CHЕМ 1112 Exp 10B.pdf 1 of 1 ENT 10.B Enthalpy PART B Heat of Reaction of Mg(s) + HCl(aq) Initial temperature of HCI solution 22. 2c Mass of magnesium Moles of magnesium moles Highest temperature of mixture 61.6 °C AT of mixture °C Heat gained by the solution J Heat lost by the reaction J Heat of reaction per mole of magnesium J/mole Mg Heat of reaction per mole of magnesium kJ/mole Mg Heat of Reaction of MgO(s) + HCI(aq) _22.0 1,011 8 Initial temperature of HCI solution °C Mass of magnesium oxide Moles of magnesium oxide moles Highest temperature of mixture 36.9 °C AT of mixture °C Heat gained by the solution J Heat lost by the reaction Heat of reaction per mole of magnesium oxide J/mole MgO Heat of reaction per mole of magnesium oxide kJ/mole MgO Heat of reaction of water -285.9 kJ/mole H;0 Heat of reaction per mole of magnesium (from previous section) kJ/mole Mg AH,MgO(s) kJ/mole MgO AH,MgO(s) (Textbook value, if available, for comparison] kJ/mole MgO 132
Transcribed Image Text:.ll T-Mobile Wi-Fi ? 2:23 PM @ O 66% f Data - CHЕМ 1112 Exp 10B.pdf 1 of 1 ENT 10.B Enthalpy PART B Heat of Reaction of Mg(s) + HCl(aq) Initial temperature of HCI solution 22. 2c Mass of magnesium Moles of magnesium moles Highest temperature of mixture 61.6 °C AT of mixture °C Heat gained by the solution J Heat lost by the reaction J Heat of reaction per mole of magnesium J/mole Mg Heat of reaction per mole of magnesium kJ/mole Mg Heat of Reaction of MgO(s) + HCI(aq) _22.0 1,011 8 Initial temperature of HCI solution °C Mass of magnesium oxide Moles of magnesium oxide moles Highest temperature of mixture 36.9 °C AT of mixture °C Heat gained by the solution J Heat lost by the reaction Heat of reaction per mole of magnesium oxide J/mole MgO Heat of reaction per mole of magnesium oxide kJ/mole MgO Heat of reaction of water -285.9 kJ/mole H;0 Heat of reaction per mole of magnesium (from previous section) kJ/mole Mg AH,MgO(s) kJ/mole MgO AH,MgO(s) (Textbook value, if available, for comparison] kJ/mole MgO 132
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