Three solutions, all originally at 20°C, are combined in a calorimeter. The temperature of the reaction mixture is monitored, as show in the graph below. 34.0- 32.0 30.0 28.0- 26.0- 24.0 22.0- 20.0 18.0 Time Ms. Prohaska repeats the same experiment, but this time she doubles the volume of each reactant, but keeps the concentration the same as in trial one. The magnitude of the molar enthalpy change calculated from the results of a second experiment is the same as the result calculated from the first experiment. Explain this result.
Three solutions, all originally at 20°C, are combined in a calorimeter. The temperature of the reaction mixture is monitored, as show in the graph below. 34.0- 32.0 30.0 28.0- 26.0- 24.0 22.0- 20.0 18.0 Time Ms. Prohaska repeats the same experiment, but this time she doubles the volume of each reactant, but keeps the concentration the same as in trial one. The magnitude of the molar enthalpy change calculated from the results of a second experiment is the same as the result calculated from the first experiment. Explain this result.
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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explain the answer using the hess's law (gr 13) please type if possible
Transcribed Image Text:Three solutions, all originally at 20°C, are combined in a calorimeter. The temperature of the reaction
mixture is monitored, as show in the graph below.
Temperature (°C)
34.0-
32.0-
30.0-
28.0-
26.0-
24.0-
22.0-
20.0-
18.0
Time
Ms. Prohaska repeats the same experiment, but
this time she doubles the volume of each
reactant, but keeps the concentration the same
as in trial one.
The magnitude of the molar enthalpy change
calculated from the results of a second
experiment is the same as the result calculated
from the first experiment. Explain this result.
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