Answer:
<u>The last statement describes the correct inozation of water:</u>
Pure water at 25ºC:
- self-ionizes to form an equilibrium system in which:
Explanation:
It has been proven that <em>pure wate</em>r slightly conducts electricity. This fact, explained by the Arrhenius model of acids, would mean that pure water contains ions.
Since such ions are spontaneoulsy produced by the water molecules, this phenomenum is called <em>self-ionization of water</em>.
The equilibrium equation that represents the self-ionization of water is:
The expression for the equilibrium constant is:
As per the stoichiometry:
The equilibrium constant for the self-ionization of water has been determined at several temperatures. At 25ºC it is equal to 1.0×10⁻¹⁴.
Then by solving the equation you can find the concentrations of the ions:
Hence, we have proved that pure water self-ionizes to form an equilibrium system in which:
By Gayle-Lussac's law, the pressure and temperature of a fixed volume and amount of gas is directly proportional.
Thus,
P/T = constant
So if the temperature is increased four times, the pressure is also increased four times.
Answer:
The correct option is d.
Explanation:
The reaction in the question is that for the formation of ammonia. The arrow in the reaction should be a reversible arrow. Because of the negative ΔH value, the forward reaction is exothermic while the reverse reaction is endothermic.
An increase in temperature of a system at equilibrium favors the endothermic reaction, hence the reverse reaction (the reactants) is favored. And when the reverse reaction is favored, more reactants are produced. Hence, product formation (at equilibrium) is not favored as the temperature is raised.