A 34.3 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter containing a certain mass of water. If the temperature rose from 35.0 to 76.7°C, how much water, in kg, must the bomb calorimeter have contained? The molar mass of ethanol is 46.07 g/mol. Assume that the calorimeter doesn't absorb any
A 34.3 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter containing a certain mass of water. If the temperature rose from 35.0 to 76.7°C, how much water, in kg, must the bomb calorimeter have contained? The molar mass of ethanol is 46.07 g/mol. Assume that the calorimeter doesn't absorb any
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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A 34.3 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter containing a certain mass of water. If the temperature rose from 35.0 to 76.7°C, how much water, in kg, must the bomb calorimeter have contained? The molar mass of ethanol is 46.07 g/mol. Assume that the calorimeter doesn't absorb any heat. The specific heat of water is 4.184 J/g °C.
C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(g) ΔH°rxn = -1.24 x 103 kJ/mol
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