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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.

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.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section4.8: Measuring Reaction Enthalpies: Calorimetry
Problem 4.17E
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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.
Transcribed Image Text: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.
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