When 0.850 g of C was burned in oxygen in a constant volume calorimeter, 27.9 kJ of energy as heat was evolved. The calorimeter was in an insulated container with 370. g of water at an initial temperature of 16.8 °C. The heat capacity of the bomb in the calorimeter is 800. J/K. The specific heat capacity of water is 4.184 J/g °C. a Calculate AU for the oxidation of C (in kJ/mol C). kJ/mol C AU =

When 0.850 g of C was burned in oxygen in a constant volume calorimeter, 27.9 kJ of energy as heat was evolved. The calorimeter was in an insulated container with 370. g of water at an initial temperature of 16.8 °C. The heat capacity of the bomb in the calorimeter is 800. J/K. The specific heat capacity of water is 4.184 J/g °C. a Calculate AU for the oxidation of C (in kJ/mol C). kJ/mol C AU =

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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In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.00 mL of 1.00 M HCl are mixed. Both solutions were originally at 24.6 C. After the reaction, the final temperature is 31.3 C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87, calculate the change in enthalpy of neutralization per mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.
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22. A 44.97−g sample of water at 72.2°C is added to a sample of water at 25.7°C in a constant-pressure calorimeter. If the final temperature of the combined water is 38.4°C and the heat capacity of the calorimeter is 26.3 J/°C, calculate the mass of the water originally in the calorimeter.
In a coffee cup calorimeter, 50.0 mL of 1.00 M NaOH and 50.0 rnL of 1.00 M HCI are mixed. Both solutions were originally at 24.6 °C. After the reaction, the final temperature is 31.3 °C. Given that the density of NaCl solution is 1.038 g/mL and the specific heat of NaCl solution is 3.87 J/g-°C, calculate the ΔHneut/mole for the reaction of HCl with NaOH. Assume that no heat is lost to the surroundings.
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When 0.900 g of Mg was burned in oxygen in a constant volume calorimeter, 22.3 kJ of energy as heat was evolved. The calorimeter was in an insulated container with 880. g of water at an initial temperature of 13.4 °C. The heat capacity of the bomb in the calorimeter is 660. J/K. The specific heat capacity of water is 4.184 J/g °C. a Calculate AU for the oxidation of Mg (in kJ/mol Mg). AU = -597.67 kJ/mol Mg The amount of heat that would evolve from burning of 1 mole of Mg should be calculated: 24.31 g/mol Mg 0.900 g AU = 9r - 22.3 kJ x == Correct - 602 kJ/mol Mg °C b what will be the final temperature of the water and the bomb calorimeter in this experiment? Final temperature =
1. Magnesium solid reacts with aqueous hydrochloric acid to form the Mg2+ ion in solution. In an experiment, 60.0 mL of aqueous HCl was mixed with 0.1297 g of magnesium solid in a double Styrofoam cup calorimeter. The reaction caused the temperature of the substances in the calorimeter to rise 10.02°C. Assume the density and specific heat of the HCl solution is that of water, 1.00 g/mL and 4.184 J/g °C, respectively. The specific heat of magnesium is 1.02 J/g °C. a. Write the balanced chemical equation for this reaction. b. Calculate the heat of this reaction, AHrxn, in kJ. c. Calculate the heat of this reaction per mole of Mg2+ formed, AHxn/mole Mg²+. d. The literature value of this reaction is -466.85 kJ/mole. Calculate the percent deviation of the experimental value from the literature value.