If a student used a sample of metal that was wet, several percent of the apparent mass of the metal would be water. Would you expect the resulting measured value of the heat capacity to be too high or too low? Explain.

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Calorimetry of metals
Prelab
1. If a student used a sample of metal that was wet, several percent of the apparent mass of the
metal would be water. Would you expect the resulting measured value of the heat capacity to
be too high or too low? Explain.
2. A particular metal element, M, has a heat capacity of 0.36 J/g K, and it forms an oxide that
contains 2.90 g M per g 0.
a. Using the law of Dulong and Pettit (S x M = 25 J/ mol K), estimate the molar mass of the
metal M.
g/mol
b. From the composition of the oxide (2.90 g M/g O) and the molar mass of O, determine the
mass of M that combines with each moles of oxygen.
g M/ mol O
Use your estimate of the atomic mass form (a) and the information from (b) to determine the
empirical formula of the oxide.
C.
d. Now that you know the composition of the oxide and its formula, what is the accurate value of
the atomic mass of the metal M? What is the likely identity of M?
g/mol
identity
Transcribed Image Text:Calorimetry of metals Prelab 1. If a student used a sample of metal that was wet, several percent of the apparent mass of the metal would be water. Would you expect the resulting measured value of the heat capacity to be too high or too low? Explain. 2. A particular metal element, M, has a heat capacity of 0.36 J/g K, and it forms an oxide that contains 2.90 g M per g 0. a. Using the law of Dulong and Pettit (S x M = 25 J/ mol K), estimate the molar mass of the metal M. g/mol b. From the composition of the oxide (2.90 g M/g O) and the molar mass of O, determine the mass of M that combines with each moles of oxygen. g M/ mol O Use your estimate of the atomic mass form (a) and the information from (b) to determine the empirical formula of the oxide. C. d. Now that you know the composition of the oxide and its formula, what is the accurate value of the atomic mass of the metal M? What is the likely identity of M? g/mol identity
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