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

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: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter15: Energy And Chemical Change

Section: Chapter Questions

Problem 112A: sample of natural gas is analyzed and found to be88.4% methane (CH4) and 11.6% ethane (C2H6) bymass....

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Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
The enthalpy of vaporization for water is 40.65 kJ mol-1. As a design engineer for a project in a desert climate, you are exploring the option of using evaporative cooling. (a) If the air has an average volumetric heat capacity of 0.00130 J cm-3 K-1, what is the minimum mass of water that would need to evaporate in order to cool a 5 m? 5 m room with a 3 m ceiling by 5°F using this method? (b) Is this a spontaneous or nonspontaneous process?
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sample of natural gas is analyzed and found to be88.4% methane (CH4) and 11.6% ethane (C2H6) bymass. The standard enthalpy of combustion of methaneto gaseous carbon dioxide (CO2) and liquid water (H2O) is -891 kJ/mol. Write the equation for the combustionof gaseous ethane to carbon dioxide and water.Calculate the standard enthalpy of combustion of ethaneusing standard enthalpies of formation from Table R-11on page 975. Using that result and the standard enthalpyof combustion of methane in Table 15.3, calculate theenergy released by the combustion of 1 kg of natural gas.