If 2.00 moles of propanol, C3H3O, needed to absorb 110.0 kJ of heat to be vaporized at 97.0 °C (the boiling point), then what was the initial temperature of the propanol? C3H&O(1) → C3H&O(g) AHvan = +47.5 kJ/mole C,(C,H,O) = 2.40 J/g.°C
Electronic Effects
The effect of electrons that are located in the chemical bonds within the atoms of the molecule is termed an electronic effect. The electronic effect is also explained as the effect through which the reactivity of the compound in one portion is controlled by the electron repulsion or attraction producing in another portion of the molecule.
Drawing Resonance Forms
In organic chemistry, resonance may be a mental exercise that illustrates the delocalization of electrons inside molecules within the valence bond theory of octet bonding. It entails creating several Lewis structures that, when combined, reflect the molecule's entire electronic structure. One Lewis diagram cannot explain the bonding (lone pair, double bond, octet) elaborately. A hybrid describes a combination of possible resonance structures that represents the entire delocalization of electrons within the molecule.
Using Molecular Structure To Predict Equilibrium
Equilibrium does not always imply an equal presence of reactants and products. This signifies that the reaction reaches a point when reactant and product quantities remain constant as the rate of forward and backward reaction is the same. Molecular structures of various compounds can help in predicting equilibrium.
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Interpretation:
Propanol is initially at some temperature and upon absorption of energy the temperature change to which is its boiling point. Complete propanol has got vaporized (changed from liquid to gas ).
As energy is absorbed by propanol, it is clear than initial temperature is less than as absorption of energy results in increase of temperature.
This conversion involves two processes in which energy is absorbed. They are:
- Energy required to attain temperature from initial temperature.
- Energy required to vaporize propanol.
To determine the initial temperature of propanol the energy involved in raising the temperature is determined by substracting the energy required for vaporization from total energy absorbed.
Given that,
Moles of propanol = 2.00
Positive sign denotes that the energy is absorbed by the system.
There are two moles of propanol present and 47.5 kJ of energy is absorbed for each mole to get vaporize.
So, for 2 moles of propanol the energy required is = 2 x 47.5 kJ = 95 kJ
Therefore, 95 kJ of energy is required to vaporize 2 moles of propanol.
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