A sample of solid 1,9-nonanediol (C9H20O2) that weighs 0.5724 g is burned in an excess of oxygen to CO2(g) and H2O(l) in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.210 °C. The heat capacity of the calorimeter and its contents is known to be 9.268×10^3 J K^-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Please specify states such as (aq) or (s).
____+____--->____+____
Based on this experiment: (b) Assuming that H° is approximately equal to E, calculate the standard enthalpy change for the combustion of 1.000 mol of 1,9-nonanediol to CO2(g) and H2O(l).
____ kJ mol-1
(c) Calculate the standard enthalpy of formation per mole of 1,9-nonanediol, using the following for the standard enthalpies of formation of CO2(g) and H2O(l).
Hf° H2O (l) = -285.83 kJ mol-1 ; Hf° CO2(g) = -393.51 kJ mol-1
____ kJ mol-1
A sample of solid 1,9-nonanediol (C9H20O2) that weighs 0.5724 g is burned in an excess of...
A sample of solid bianthracene (C28H18) that weighs 0.5275 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.170 °C. The heat capacity of the calorimeter and its contents is known to be 9.520×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Based on this experiment: (b) Assuming that H° is approximately equal...
A sample of solid 1,2-benzenediol (C6H6O2) that weighs 0.8129 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.270 °C. The heat capacity of the calorimeter and its contents is known to be 9.301×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction.Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s)....
A sample of solid pyrene (C16H10) that weighs 0.5063 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.130 °C. The heat capacity of the calorimeter and its contents is known to be 9.233×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or...
A sample of solid diphenyl phthalate (C20H14O4) that weighs 0.6847 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.110 °C. The heat capacity of the calorimeter and its contents is known to be 9.580×103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq)...
Thermometer A sample of solid bianthracene (C28H18) that weighs 0.5254 g is burned in an excess of oxygen to CO2(g) and H2O() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.190 °C. The heat capacity of the calorimeter and its contents is known to be 9.405x103 JK. Ignition wires heat sample Stirrer (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify...
help pt) A sample of 1.0 mol of liquid octane C8H18(1) undergoes combustion accord 5. (10 pt) A C3H18(0) + O2(g) → 8 CO2(g) + 9 H2O(l) Using the standard enthalpies of formation given calculate the change in enthalpy in kJ/mol associated with the combustion of 1.0 mol of C8H18(1) at 1.0 bar pressure and 25 °C. Substance AH® (kJ/mol) C8H18() -249.9 CO2(g) -393.51 H2O) -285.83
The standard enthalpy change of combustion [to CO2(g) and H2O()] at 25°C of the organic solid para-benzoquinone, C6H4O2(s), is determined to be -2767.0 kJ mol-1. What is the Hf° of C6H4O2(s) based on this value? Use the following data: Hf° H2O () = -285.83 kJ mol-1 ; Hf° CO2(g) = -393.51 kJ mol-1 kJ mol-1
The standard enthalpy change of combustion [to CO2(g) and H2O()] at 25°C of the organic solid bianthracene, C28H18(s), is determined to be -13924.1 kJ mol-1. What is the Hf° of C28H18(s) based on this value? Use the following data: Hf° H2O () = -285.83 kJ mol-1 ; Hf° CO2(g) = -393.51 kJ mol-1 _________ kJ mol-1
For the combustion of cyclopropane at 25 ºC C3H6(g) + (9/2) O2(g) → 3 CO2(g) + 3 H2O(liq) ΔHºc(C3H6,g) = -2091 kJ / mol. What is the standard molar enthalpy of formation of cyclopropane(g) at 25 ºC if the standard molar enthalpies of formation of CO2(g) and H2O(liq) at that temperature are, respectively, -393.51 kJ / mol and -285.83 kJ / mol?
The standard molar enthalpy of combustion, deltacHm, of C2H6 (g) is -1559.8 kJ/mol. 1. Use some of the following data to calculate the molar enthalpy of formation of C2H6(g) at 298.15 K 2. Calculate the molar enthalpy of combustion of ethane at 500K Table provided gives values of standard enthalpy of formation values at 298.15 K Substance deltafH (kJ*mol^-1) Cpm (J*K^-1*mol^-1) CO2 (aq) -413.8 N/A CO2 (g) -393.51 37.11 H2O (l) -285.83 75.291 H2O(g) -241.82 33.58 C2H6(g) to be determined...