The combustion of 1.000g of naphthalene, a compound containing only carbon and hydrogen, was conducted in a bomb calorimeter with a heat capacity of 5.994 kJ/*C. It produced 3.433g of CO2 and 0.562g of H2O. The standard heat of formation of CO2 is -393.5kJ/mol and -285.9kj/mol for H2O. a. Determine the emperocal formula of the compound. b. If the compound has a molar mass if 128.17g/mol, determine the molecular formula of the compound. c. If the temperature in the calorimeter increase by 6.70*C, determine the heat release by the reaction. d. determine the standard enthalpy of formation of the compound.
The combustion of 1.000g of naphthalene, a compound containing only carbon and hydrogen, was conducted in a bomb calorimeter with a heat capacity of 5.994 kJ/*C. It produced 3.433g of CO2 and 0.562g of H2O. The standard heat of formation of CO2 is -393.5kJ/mol and -285.9kj/mol for H2O. a. Determine the emperocal formula of the compound. b. If the compound has a molar mass if 128.17g/mol, determine the molecular formula of the compound. c. If the temperature in the calorimeter increase by 6.70*C, determine the heat release by the reaction. d. determine the standard enthalpy of formation of the compound.
Chemistry
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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
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Transcribed Image Text:**Exercise on Combustion Analysis and Thermochemistry**
The combustion of 1.000 g of naphthalene, a compound containing only carbon and hydrogen, was conducted in a bomb calorimeter with a heat capacity of 5.994 kJ/°C. It produced 3.433 g of CO₂ and 0.562 g of H₂O.
The standard heat of formation of CO₂ is -393.5 kJ/mol and -285.9 kJ/mol for H₂O.
**Questions:**
a. Determine the empirical formula of the compound.
b. If the compound has a molar mass of 128.17 g/mol, determine the molecular formula of the compound.
c. If the temperature in the calorimeter increases by 6.70°C, determine the heat released by the reaction.
d. Determine the standard enthalpy of formation of the compound.
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