To a test tube containing 10.0 ml of 0.50 M HCl solution in a calorimeter, 0.05482 g of solid MgO (MW = 40.30 g/mol) at the same temperature was added. A change in temperature of 6.2°C was recorded. In a separate experiment, the heat capacity of the calorimeter was determined to be 0.293 kJ/°C. 1. Calculate the experimental ΔHrxn (in kJ/mol) for the reaction between MgO and HCl. 2. If the theoretical ΔHrxn of the reaction between MgO and HCl is -1349 kJ/mol, calculate the %error.
To a test tube containing 10.0 ml of 0.50 M HCl solution in a calorimeter, 0.05482 g of solid MgO (MW = 40.30 g/mol) at the same temperature was added. A change in temperature of 6.2°C was recorded. In a separate experiment, the heat capacity of the calorimeter was determined to be 0.293 kJ/°C. 1. Calculate the experimental ΔHrxn (in kJ/mol) for the reaction between MgO and HCl. 2. If the theoretical ΔHrxn of the reaction between MgO and HCl is -1349 kJ/mol, calculate the %error.
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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To a test tube containing 10.0 ml of 0.50 M HCl solution in a calorimeter, 0.05482 g
of solid MgO (MW = 40.30 g/mol) at the same temperature was added. A change in
temperature of 6.2°C was recorded. In a separate experiment, the heat capacity of
the calorimeter was determined to be 0.293 kJ/°C.
1. Calculate the experimental ΔHrxn (in kJ/mol) for the reaction between MgO and
HCl.
2. If the theoretical ΔHrxn of the reaction between MgO and HCl is -1349 kJ/mol,
calculate the %error.
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