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1) When a mass, m, of cyclohexane is burnt in a constant volume bomb calorimeter with heat capacity Ccal, the temperature of the water surrounding the calorimeter is raised by AТ. The heat of combustion of the nichrome wire used to ignite the reactive mixture is q. The lengths of the nichrome wire before and after combustion are Lo and L, respectively. The combustion reaction is carried out at temerature T and pressure P. The standard molar enthalpy of combustion of cyclohexane is written as A ¿H° . Table 1 Experimental conditions and thermodynamic data for AH° m Ccal q Lo L T P the combustion in the bomb calorimeter -3951 +/- 19 kJ/mol 0.78 0.002 g 8222.0+/8.0 J/k -9.6 J/cm 9. 39 +0.05 cm 3. 39 +0.05 cm 20.65 0.04 °C 25.8 +/- 1.0 bar a) Write a balanced equation for the combustion of cyclohexane. (Make sure all stoichiometric coefficients are the smallest possible integers, even if they are "1". Pay attention to phases!) (1) + (1) + (g) Δ b) Using data from Table 1 and from the lab handouts, predict the temperature rise for the water surrounding the calorimeter, ATн, and its standard deviation using the propagation of error method. (Pay attention to the number of sigificant digits used for the molar mass and the gas constant!) ATH₂O = +/- c) Given that the magnitudes of the standard molar heat of combustion of graphite and hydrogen (H2) are -285.83 and -395.51 kJ/mol respectively, determine the standard molar head of formation (A (H) of cyclohexane using the appropriate data from Table 1. (Pay attention to the signs!) A&H = +/- kJ/mol d) Given the standard molar enthalpy of formation of hexane is -167.2 kJ/mol, determine the C-C bond dissociation energy of cyclohexane. BDE (C-C) = +/- kJ/mol

1) When a mass, m, of cyclohexane is burnt in a constant volume bomb calorimeter with heat capacity Ccal, the temperature of the water surrounding the calorimeter is raised by AТ. The heat of combustion of the nichrome wire used to ignite the reactive mixture is q. The lengths of the nichrome wire before and after combustion are Lo and L, respectively. The combustion reaction is carried out at temerature T and pressure P. The standard molar enthalpy of combustion of cyclohexane is written as A ¿H° . Table 1 Experimental conditions and thermodynamic data for AH° m Ccal q Lo L T P the combustion in the bomb calorimeter -3951 +/- 19 kJ/mol 0.78 0.002 g 8222.0+/8.0 J/k -9.6 J/cm 9. 39 +0.05 cm 3. 39 +0.05 cm 20.65 0.04 °C 25.8 +/- 1.0 bar a) Write a balanced equation for the combustion of cyclohexane. (Make sure all stoichiometric coefficients are the smallest possible integers, even if they are "1". Pay attention to phases!) (1) + (1) + (g) Δ b) Using data from Table 1 and from the lab handouts, predict the temperature rise for the water surrounding the calorimeter, ATн, and its standard deviation using the propagation of error method. (Pay attention to the number of sigificant digits used for the molar mass and the gas constant!) ATH₂O = +/- c) Given that the magnitudes of the standard molar heat of combustion of graphite and hydrogen (H2) are -285.83 and -395.51 kJ/mol respectively, determine the standard molar head of formation (A (H) of cyclohexane using the appropriate data from Table 1. (Pay attention to the signs!) A&H = +/- kJ/mol d) Given the standard molar enthalpy of formation of hexane is -167.2 kJ/mol, determine the C-C bond dissociation energy of cyclohexane. BDE (C-C) = +/- kJ/mol

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ISBN:9781305957404
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Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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1) When a mass, m, of cyclohexane is burnt in a constant volume bomb calorimeter with heat capacity Ccal, the temperature of the water surrounding the calorimeter is raised by AТ. The heat of combustion of the nichrome wire used to ignite the reactive mixture is q. The lengths of the nichrome wire before and after combustion are Lo and L, respectively. The combustion reaction is carried out at temerature T and pressure P. The standard molar enthalpy of combustion of cyclohexane is written as A ¿H° . Table 1 Experimental conditions and thermodynamic data for AH° m Ccal q Lo L T P the combustion in the bomb calorimeter -3951 +/- 19 kJ/mol 0.78 0.002 g 8222.0+/8.0 J/k -9.6 J/cm 9. 39 +0.05 cm 3. 39 +0.05 cm 20.65 0.04 °C 25.8 +/- 1.0 bar a) Write a balanced equation for the combustion of cyclohexane. (Make sure all stoichiometric coefficients are the smallest possible integers, even if they are "1". Pay attention to phases!) (1) + (1) + (g) Δ b) Using data from Table 1 and from the lab handouts, predict the temperature rise for the water surrounding the calorimeter, ATн, and its standard deviation using the propagation of error method. (Pay attention to the number of sigificant digits used for the molar mass and the gas constant!) ATH₂O = +/- c) Given that the magnitudes of the standard molar heat of combustion of graphite and hydrogen (H2) are -285.83 and -395.51 kJ/mol respectively, determine the standard molar head of formation (A (H) of cyclohexane using the appropriate data from Table 1. (Pay attention to the signs!) A&H = +/- kJ/mol d) Given the standard molar enthalpy of formation of hexane is -167.2 kJ/mol, determine the C-C bond dissociation energy of cyclohexane. BDE (C-C) = +/- kJ/mol
Transcribed Image Text:1) When a mass, m, of cyclohexane is burnt in a constant volume bomb calorimeter with heat capacity Ccal, the temperature of the water surrounding the calorimeter is raised by AТ. The heat of combustion of the nichrome wire used to ignite the reactive mixture is q. The lengths of the nichrome wire before and after combustion are Lo and L, respectively. The combustion reaction is carried out at temerature T and pressure P. The standard molar enthalpy of combustion of cyclohexane is written as A ¿H° . Table 1 Experimental conditions and thermodynamic data for AH° m Ccal q Lo L T P the combustion in the bomb calorimeter -3951 +/- 19 kJ/mol 0.78 0.002 g 8222.0+/8.0 J/k -9.6 J/cm 9. 39 +0.05 cm 3. 39 +0.05 cm 20.65 0.04 °C 25.8 +/- 1.0 bar a) Write a balanced equation for the combustion of cyclohexane. (Make sure all stoichiometric coefficients are the smallest possible integers, even if they are "1". Pay attention to phases!) (1) + (1) + (g) Δ b) Using data from Table 1 and from the lab handouts, predict the temperature rise for the water surrounding the calorimeter, ATн, and its standard deviation using the propagation of error method. (Pay attention to the number of sigificant digits used for the molar mass and the gas constant!) ATH₂O = +/- c) Given that the magnitudes of the standard molar heat of combustion of graphite and hydrogen (H2) are -285.83 and -395.51 kJ/mol respectively, determine the standard molar head of formation (A (H) of cyclohexane using the appropriate data from Table 1. (Pay attention to the signs!) A&H = +/- kJ/mol d) Given the standard molar enthalpy of formation of hexane is -167.2 kJ/mol, determine the C-C bond dissociation energy of cyclohexane. BDE (C-C) = +/- kJ/mol
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