A student tries to calculate the enthalpy of reaction for an acid-base reaction. 1.0 M HBr and 1.0 M KOH is used for the reaction shown below. Which of the following mistakes would cause the smallest deviation from the true value? O The final temperature of the mixture was taken before the contents of the calorimeter had reached thermal equilibrium. O The actual molarity of the base solution was 1.1 M but was recorded as 1.0 M. O The thermometer was incorrectly calibrated and read 2.0 Celsius degree too high during the procedure. O The volume of the acid solution added to the calorimeter was actually 0.5 mL less than what was recorded. The calorimeter was poorly insulated, and some heat escaped to the atmosphere during the procedure.
A student tries to calculate the enthalpy of reaction for an acid-base reaction. 1.0 M HBr and 1.0 M KOH is used for the reaction shown below. Which of the following mistakes would cause the smallest deviation from the true value? O The final temperature of the mixture was taken before the contents of the calorimeter had reached thermal equilibrium. O The actual molarity of the base solution was 1.1 M but was recorded as 1.0 M. O The thermometer was incorrectly calibrated and read 2.0 Celsius degree too high during the procedure. O The volume of the acid solution added to the calorimeter was actually 0.5 mL less than what was recorded. The calorimeter was poorly insulated, and some heat escaped to the atmosphere during the procedure.
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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Transcribed Image Text:A student tries to calculate the enthalpy of reaction for an acid-base reaction. 1.0 M HBr and 1.0 M KOH is used for the reaction shown below. Which of
the following mistakes would cause the smallest deviation from the true value?
The final temperature of the mixture was taken before the contents of the calorimeter had reached thermal equilibrium.
The actual molarity of the base solution was 1.1 M but was recorded as 1.0 M.
The thermometer was incorrectly calibrated and read 2.0 Celsius degree too high during the procedure.
The volume of the acid solution added to the calorimeter was actually 0.5 mL less than what was recorded.
The calorimeter was poorly insulated, and some heat escaped to the atmosphere during the procedure.
Transcribed Image Text:A student conducted a precipitation experiment for Mg(OH)2 (s) by mixing 250 mL of 0.5 M MgCl2 (aq) and a 250 mL of 1.0 M NaOH (aq). If the student
wants to repeat the experiment to produce the same final volume but double the amount of precipitate produced, which of the following changes should
they make to the procedure?
MgCl2 (aq) + 2 NaOH (aq) → 2 NaCI (aq) + Mg(OH)2 (s)
O Using twice the molarity of MgCl2 (aq) and twice the molarity of NaOH (aq)
Using the same molarity of MgCl2 (aq) but twice the molarity of NaOH (aq)
O Using twice the molarity of MgCl2 (aq) but the same molarity of NaOH (aq)
Using twice the molarity of MgCl2 (aq) but half the molarity of NaOH (aq)
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