A sample of solid glutaric acid (C5H3O4) that weighs 1.245 g is burned in an excess of Ignition wires heat oxygen to Thermometer CO2(g) and H20() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be Stirrer 2.190 °C. The heat capacity of the calorimeter and its contents is known to be 9.242×10³ J K-!. sample (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). If a box is not needed, leave it blank. Water Based on this experiment: (b) Assuming that AH° is approximately equal to AE, calculate the standard enthalpy change for the combustion of 1.000 mol of glutaric acid to CO2(g) and H20(). Insulated outside chamber Sample dish Burning sample Steel bomb kJ mol-1 Combustion (bomb) calorimeter. (c) Calculate the standard enthalpy of formation per mole of glutaric acid, using the following for the standard enthalpies of formation of CO2(g) and H2O(g). AH° H20 (2)=-285.83 kJ mol-! ; AHº CO2(g) =-393.51 kJ mol-1 kJ mol-!
A sample of solid glutaric acid (C5H3O4) that weighs 1.245 g is burned in an excess of Ignition wires heat oxygen to Thermometer CO2(g) and H20() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be Stirrer 2.190 °C. The heat capacity of the calorimeter and its contents is known to be 9.242×10³ J K-!. sample (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). If a box is not needed, leave it blank. Water Based on this experiment: (b) Assuming that AH° is approximately equal to AE, calculate the standard enthalpy change for the combustion of 1.000 mol of glutaric acid to CO2(g) and H20(). Insulated outside chamber Sample dish Burning sample Steel bomb kJ mol-1 Combustion (bomb) calorimeter. (c) Calculate the standard enthalpy of formation per mole of glutaric acid, using the following for the standard enthalpies of formation of CO2(g) and H2O(g). AH° H20 (2)=-285.83 kJ mol-! ; AHº CO2(g) =-393.51 kJ mol-1 kJ mol-!
Chemistry: Principles and Practice
3rd Edition
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Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
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Transcribed Image Text:A sample of solid glutaric acid (C5H3O4) that weighs 1.245 g is burned in an excess of
Ignition
wires
heat
oxygen to
Thermometer
CO2(g) and H20() in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be
Stirrer
2.190 °C. The heat capacity of the calorimeter and its contents is known to be 9.242×10³ J K-!.
sample
(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). If a box is not needed, leave it
blank.
Water
Based on this experiment:
(b) Assuming that AH° is approximately equal to AE, calculate the standard enthalpy change for the
combustion of 1.000 mol of glutaric acid to CO2(g) and H20().
Insulated
outside
chamber
Sample
dish
Burning
sample
Steel
bomb
kJ mol-1
Combustion (bomb) calorimeter.
(c) Calculate the standard enthalpy of formation per mole of glutaric acid, using the following for the standard enthalpies of formation of CO2(g) and
H2O(g).
AH° H20 (2)=-285.83 kJ mol-! ; AHº CO2(g) =-393.51 kJ mol-1
kJ mol-!
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