Concept explainers
Interpretation:
An explanation about the sublimation enthalpy of ice at
Concept Introduction:
If a transition or process is taking place where the initial and final state of the substance are different, then the formula for calculating the heat required for the process is given below.
Where,
Explanation of Solution
The heat capacity of liquid water and water vapor are
The heat energy required to heat up one mole of liquid water by
Similarly, the heat energy required to heat up one mole of water vapor by
Four required thermochemical processes that sum to produce form the sublimation equation of water is given below.
This result is quite close to the
The heat capacity of liquid
The heat energy required to heat up one mole of liquid
Similarly, the heat energy required to heat up one mole of
The heat energy required to heat up one mole of liquid
Similarly, the heat energy required to heat up one mole of
For
Fusion enthalpy of
For
Fusion enthalpy of
Therefore, the sublimation enthalpies of
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Chapter 9 Solutions
Chemistry: The Molecular Science
- Calculate the quantity of heating required to convert the water in four ice cubes (60.1 g each) from H2O(s) at 0 °C to H2O(g) at 100. °C. The enthalpy of fusion of ice is 333 J/g and the enthalpy of vaporization of liquid water is 2260 J/g.arrow_forwardWhy are steam burns so much worse than water burns even if the H2O is at the same temperature for both phases? Hint: Consider the heat of vaporization of water.arrow_forwardConsider the phase diagram and heating-curve graphs for Question 113. Draw corresponding heating curves for T1 to T2 at pressures P1 and P2. Label each phase and phase change on your heating curves.arrow_forward
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- The cooling effect of alcohol on the skin is due to its evaporation. Calculate the heat of vaporization of ethanol (ethyl alcohol), C2H5OH. C2H5OH(l)C2H5OH(g);H=? The standard enthalpy of formation of C2H5OH(l) is 277.7 kJ/mol and that of C2H5OH(g) is 235.1 kJ/mol.arrow_forwardLiquid butane, C4H10, is stored in cylinders to be used as a fuel. Suppose 35.5 g of butane gas is removed from a cylinder. How much heat must be provided to vaporize this much gas? The heat of vaporization of butane is 21.3 kJ/mol.arrow_forward
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