In determining the heat of neutralization of 50.0 mL of 1.00 M H2SO4 and 50.0 mL of 1.00 M NaOH, a student measures the initial temperatures of the sulfuric acid and sodium hydroxide solutions to be 22.5 C and 21.9 C, respectively. If the final temperature of the mixture (after the reaction) is 28.8
In determining the heat of neutralization of 50.0 mL of 1.00 M H2SO4 and 50.0 mL of 1.00 M NaOH, a student measures the initial temperatures of the sulfuric acid and sodium hydroxide solutions to be 22.5 C and 21.9 C, respectively. If the final temperature of the mixture (after the reaction) is 28.8
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 determining the heat of
neutralization of 50.0 mL of 1.00 M
H2SO4 and 50.0 mL of 1.00 M NaOH, a
student measures the initial
temperatures of the sulfuric acid and
sodium hydroxide solutions to be 22.5
C and 21.9
C, respectively. If the final temperature
of the mixture (after the reaction) is
28.8
C, calculate the molar enthalpy of this
reaction, in kJ/mol.
54 kJ/mol
O -2.7 kJ/mol
-54 kJ/mol
2.7 kJ/mol](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2a28f70d-2b7b-4d40-8264-aa0ee87b0e68%2F8ac93a0f-b227-4bb8-973c-a5f0319f484a%2Fu5uc1oy_processed.png&w=3840&q=75)
Transcribed Image Text:In determining the heat of
neutralization of 50.0 mL of 1.00 M
H2SO4 and 50.0 mL of 1.00 M NaOH, a
student measures the initial
temperatures of the sulfuric acid and
sodium hydroxide solutions to be 22.5
C and 21.9
C, respectively. If the final temperature
of the mixture (after the reaction) is
28.8
C, calculate the molar enthalpy of this
reaction, in kJ/mol.
54 kJ/mol
O -2.7 kJ/mol
-54 kJ/mol
2.7 kJ/mol
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