Answer:
c. ΔH° is positive and ΔS° is positive.
Explanation:
Hello,
In this case, as the Gibbs free energy for a reaction is defined in terms of the change in the enthalpy and entropy as shown below:
Thus, as the reaction becomes spontaneous (ΔG°<0) at temperatures above 1100K (high temperatures), it necessary that c. ΔH° is positive and ΔS° is positive as the entropy will drive the spontaneousness as it becomes smaller than TΔS°.
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Single Replacement and Double Replacement reactions
Explanation:
Just a few things to remember:
-
# of neutrons = Mass number - # protons
-
Mass number = # protons + # neutrons
-
Atomic Number = # of protons
- # of electrons = # of protons - charge on the atom
-
Symbol - use the atomic number to find the element in the periodic table
The water will boil at C) 80°C
<h3>Further explanation</h3>
Given
Vapour pressure of water = 47 kPa
Required
Boiling point of water
Solution
We can use the Clausius-Clapeyron equation :
Vapour pressure of water at boiling point 100°C=101.325 kPa
ΔH vap for water at 100°C=40657 J/mol
R = 8.314 J/mol K
T₁=boiling point of water at 101.325 kPa = 100+273=373 K
Input given values :
