A sample of solid isophthalic acid (CgH604) that weighs 1.009 g is burned in an excess of oxygen to CO2(g) and H2O(e) in a constant-volume calorimeter at 25.000°C. The temperature rise is observed to be 2.030°C. The heat capacity of the calorimeter and its contents is known to be 9593 J K¹. Ignition wires Thermometer Stirrer heat sample Water Insulated Sample Burning Steel sample bomb outside dish chamber Combustion (bomb) calorimeter. (a) Write and balance the chemical equation for the combustion reaction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) Based on this experiment: (b) Calculate the standard change in internal energy (AU) for the combustion of 1.000 mol of isophthalic acid to CO2(g) and H₂O(e). kj mol-1 (c) Calculate the standard enthalpy change (AH) for the same reaction as in part (b). kj mol-1 (d) Calculate the standard enthalpy of formation per mole of isophthalic acid, using the following for the standard enthalpies of formation of CO2(g) and H2O(l): AH°(H₂O(e)) = -285.83 kJ mol¹ and AH°(CO2(g))=-393.51 kJ mol 1 kJ mol-1

Chemistry: The Molecular Science
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Author:John W. Moore, Conrad L. Stanitski
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Chapter4: Energy And Chemical Reactions
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A sample of solid isophthalic acid (CgH604) that weighs 1.009 g is burned in an excess of oxygen to CO2(g) and H2O(e) in a constant-volume calorimeter at 25.000°C. The temperature rise is observed to be 2.030°C. The heat
capacity of the calorimeter and its contents is known to be 9593 J K¹.
Ignition
wires
Thermometer
Stirrer
heat
sample
Water
Insulated
Sample Burning Steel
sample bomb
outside dish
chamber
Combustion (bomb) calorimeter.
(a) Write and balance the chemical equation for the combustion reaction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)
Based on this experiment:
(b) Calculate the standard change in internal energy (AU) for the combustion of 1.000 mol of isophthalic acid to CO2(g) and H₂O(e).
kj mol-1
(c) Calculate the standard enthalpy change (AH) for the same reaction as in part (b).
kj mol-1
(d) Calculate the standard enthalpy of formation per mole of isophthalic acid, using the following for the standard enthalpies of formation of CO2(g) and H2O(l): AH°(H₂O(e)) = -285.83 kJ mol¹ and AH°(CO2(g))=-393.51 kJ mol
1
kJ mol-1
Transcribed Image Text:A sample of solid isophthalic acid (CgH604) that weighs 1.009 g is burned in an excess of oxygen to CO2(g) and H2O(e) in a constant-volume calorimeter at 25.000°C. The temperature rise is observed to be 2.030°C. The heat capacity of the calorimeter and its contents is known to be 9593 J K¹. Ignition wires Thermometer Stirrer heat sample Water Insulated Sample Burning Steel sample bomb outside dish chamber Combustion (bomb) calorimeter. (a) Write and balance the chemical equation for the combustion reaction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) Based on this experiment: (b) Calculate the standard change in internal energy (AU) for the combustion of 1.000 mol of isophthalic acid to CO2(g) and H₂O(e). kj mol-1 (c) Calculate the standard enthalpy change (AH) for the same reaction as in part (b). kj mol-1 (d) Calculate the standard enthalpy of formation per mole of isophthalic acid, using the following for the standard enthalpies of formation of CO2(g) and H2O(l): AH°(H₂O(e)) = -285.83 kJ mol¹ and AH°(CO2(g))=-393.51 kJ mol 1 kJ mol-1
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