When 5.00 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of 80.1°C, 169.5 kJ are
absorbed and PΔV for the vaporization process is equal to 14.5 kJ.
What is the change of internal energy?
What is the change of enthalpy?
Is the change in entropy positive or negative for this process?
If the pressure would be only ½ atm, what are the changes of internal energy and enthalpy during vaporization (approximately)?
How much energy is absorbed?
Write the definition of the Gibbs Free Energy.
At the lower pressure, will the boiling point be higher or lower.
What is the change of internal energy?
What is the change of enthalpy?
Is the change in entropy positive or negative for this process?
If the pressure would be only ½ atm, what are the changes of internal energy and enthalpy during vaporization (approximately)?
How much energy is absorbed?
Write the definition of the Gibbs Free Energy.
At the lower pressure, will the boiling point be higher or lower.
1 answer:
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Answer:
Explanation:
The definition of acids and bases by Arrhenius Theory was modified and extended by Bronsted-Lowry.
Bronsted-Lowry defined acid as a molecule or ion which donates a proton while a base is a molecule or ions that accepts the proton. This definition can be extended to include acid -base titrations in non-aqueous solutions.
In this theory, the reaction of an acid with a base constitutes a transfer of a proton from the acid to the base.
From the given information:
From above:
We will see that HCN releases an H⁺ ion, thus it is a Bronsted-Lowry acid
accepts the H⁺ ion ,thus it is a Bronsted-Lowry base.
The formula of the reactant that acts as a proton donor is <u>HCN</u>
The formula of the reactant that acts as a proton acceptor is <u>H2O</u>