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Atkins & de Paula: Elements of Physical Chemistry 5e
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In an experiment to determine its enthalpy of vaporization, liquid tetrachloromethane, CCl4, was placed in an open boiler that was equipped with a resistive heating coil and brought to the boil at a constant temperature of 350 K and pressure of 1 bar. The passage of a current of 0.933 A from a 24.0 V supply for 30.0 s was found to result in the vaporization of 3.45 g of tetrachloromethane. Calculate the standard enthalpy of vaporization of tetrachloromethane at 350 K.
For iodine, I2, at 114°C, the standard enthalpy of fusion is 16.1 kJ mol-1 and the standard enthalpy of vaporization is 45.0 kJ mol-1. Calculate the standard enthalpy of sublimation at this temperature.
The energy released as heat when liquid propanone, CH3COCH3, is burned in a bomb calorimeter at 298.15 K is 1788 kJ mol-1. Calculate the enthalpy of combustion of propanone.
Calculate the standard enthalpy of combustion of phenol, C6H5OH, at 298.15 K given that, at this temperature, the standard enthalpy of formation of phenol is -165.0 kJ mol-1, of liquid water, H2O is -285.8 kJ mol-1 and gaseous carbon dioxide, CO2, is -393.51 kJ mol-1.
Estimate the standard enthalpy change for the process F2(g) + 2 e-(g) → 2 F-(g) The F-F bond enthalpy is +155 kJ mol-1 and the electron gain enthalpy of elemental fluorine, F, is -328 kJ mol-1.
Estimate the standard enthalpy change for the reaction N2(g) + 3 H2(g) → 2 NH3(g) given the following mean bond enthalpies: H-H: +436 kJ mol-1, N-N: +945 kJ mol-1 and H-N: +388 kJ mol-1.
Estimate the standard enthalpy of formation of liquid benzene, C6H6, at 298.15 K. At this temperature, the standard enthalpy of atomization of carbon C(s, graphite) → C(g) is +717 kJ mol-1 and the standard enthalpy of vaporization of benzene is 34 kJ mol-1, whilst the standard bond enthalpy of hydrogen, H2, is 436 kJ mol-1. The mean bond enthalpy of a C6H5-H bond is 469 kJ mol-1 and of an aromatic C-C bond is 452 kJ mol-1.
Use the following data to calculate the mean B-Cl bond enthalpy in boron trichloride, BCl3.
Calculate the standard enthalpy change for the hydrogenation reaction C2H4(g) + H2(g) → C2H6(g) at 298.15 K. At this temperature, the standard enthalpy of combustion of ethene, C2H4, is -1409 kJ mol-1, of hydrogen, H2, is -286 kJ mol-1 and of ethane, C2H6 is -1560 kJ mol-1.
The standard enthalpy of combustion of propane, C3H8, is -2.220 × 103 kJ mol-1 at 400 K. Use the data below, and Kirchoff's law, to calculate the standard enthalpy of combustion at 600 K.
