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A piece of copper metal whose mass is 3.45 g is heated to 95.0°C and then dropped onto a calorimeter made of ice at 0.0°C. As the metal cools to 0.0°C, 0.372 g of the ice melts (AH (water)=6.01 kJ/mol). From this experiment, find the molar heat capacity (in J/°C*mol) of the copper. fus

A piece of copper metal whose mass is 3.45 g is heated to 95.0°C and then dropped onto a calorimeter made of ice at 0.0°C. As the metal cools to 0.0°C, 0.372 g of the ice melts (AH (water)=6.01 kJ/mol). From this experiment, find the molar heat capacity (in J/°C*mol) of the copper. fus

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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1. When 1 mol of a fuel is burned at constant pressure, it produces 3452 kJ of heat and does 11 kJ of work. What are the values of ΔΕ and ΔΗ? 2. A gas is compressed from an initial volume of 5.55 L to a final volume of 1.22L at an external pressure of 1.00 atm. During the compression, 124 J of heat are released. What is the AE (in J)? 3. A piece of copper metal whose mass is 3.45 g is heated to 95.0°C and then dropped onto a calorimeter made of ice at 0.0°C. As the metal cools to 0.0°C, 0.372 g of the ice melts (AH (water)=6.01 kJ/mol). From this experiment, find the molar heat capacity (in J/°C*mol) of the copper. 4. In order to measure the enthalpy change for the reaction that occurs in instant cold packs used by athletes, 1.25 g of NH NO, is dissolved in enough water to make 25.0 mL of solution. Th initial temperature is 25.8°C and the fina temperature is 21.9°C. Calculate the AH for the dissolution reaction below in kJ/mol. Assume that the specific heat capacity of the solution is 4.18 J/g*°C and that its density 1.00 g/mL and that the calorimeter itself absorbs a negligible amount of heat. NH4NO3(s) à NH4+ (aq) + NO₂ (aq) 5. When 0.514 g of biphenyl (CH) undergoes combustion in a bomb calorimeter, the temperature rises from 25.8°C to 29.4°C. Find the AE for the combustion of biphenyl in kJ/mol biphenyl. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.86 kJ/°C. 6. Use Hess's Law and the following data: Sro(s) à Sr (s) + 1/20₂(g) SrO(s) + CO₂(g) à SrCO3(s) 2 CO₂(g) à 2 C(graphite) + 2 O₂(g) AH°= +592 kJ AH°= -234kJ AH°=+788 kJ to determine the standard heat of formation AH (in kJ) for strontium carbonate (SrCO3). Strontium carbonate emits a brilliant red colour in flames and due to its low cost, is used in fireworks.
Transcribed Image Text:1. When 1 mol of a fuel is burned at constant pressure, it produces 3452 kJ of heat and does 11 kJ of work. What are the values of ΔΕ and ΔΗ? 2. A gas is compressed from an initial volume of 5.55 L to a final volume of 1.22L at an external pressure of 1.00 atm. During the compression, 124 J of heat are released. What is the AE (in J)? 3. A piece of copper metal whose mass is 3.45 g is heated to 95.0°C and then dropped onto a calorimeter made of ice at 0.0°C. As the metal cools to 0.0°C, 0.372 g of the ice melts (AH (water)=6.01 kJ/mol). From this experiment, find the molar heat capacity (in J/°C*mol) of the copper. 4. In order to measure the enthalpy change for the reaction that occurs in instant cold packs used by athletes, 1.25 g of NH NO, is dissolved in enough water to make 25.0 mL of solution. Th initial temperature is 25.8°C and the fina temperature is 21.9°C. Calculate the AH for the dissolution reaction below in kJ/mol. Assume that the specific heat capacity of the solution is 4.18 J/g*°C and that its density 1.00 g/mL and that the calorimeter itself absorbs a negligible amount of heat. NH4NO3(s) à NH4+ (aq) + NO₂ (aq) 5. When 0.514 g of biphenyl (CH) undergoes combustion in a bomb calorimeter, the temperature rises from 25.8°C to 29.4°C. Find the AE for the combustion of biphenyl in kJ/mol biphenyl. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.86 kJ/°C. 6. Use Hess's Law and the following data: Sro(s) à Sr (s) + 1/20₂(g) SrO(s) + CO₂(g) à SrCO3(s) 2 CO₂(g) à 2 C(graphite) + 2 O₂(g) AH°= +592 kJ AH°= -234kJ AH°=+788 kJ to determine the standard heat of formation AH (in kJ) for strontium carbonate (SrCO3). Strontium carbonate emits a brilliant red colour in flames and due to its low cost, is used in fireworks.
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