With an increase in temperature, the particles gain kinetic energy and move faster. (The ANSWER is increase the temperature.)
Answer:
1.758 x 10⁻¹¹.
Explanation:
∵ pH = - log[H⁺].
∴ 5.47 = -log[H⁺].
log[H⁺] = -5.47.
∴ [H⁺] = 3.388 x 10⁻⁶ M.
∵ [H⁺] = √(Ka.C)
∴ [H⁺]² = Ka.C
<em>∴ Ka = [H⁺]²/C </em>= (3.388 x 10⁻⁶)²(0.653) = <em>1.758 x 10⁻¹¹.</em>
Answer:
not a solid/ dissolved in water/ through melting because the ion's electrons have to be able to move freely and they can't do this when they are solids. they can occur
Answer:
The value of Gibbs free energy of the reaction is negative which means that reaction is spontaneous.
Explanation:
ΔG° = ΔH° - TΔG°
Where:
ΔG° = Change in Gibbs free energy at T temperature
ΔH° = Enthalpy of reaction at T temperature
ΔS° = Entropy change of reaction at T temperature
- The reaction with negative value of Gibbs free energy are spontaneous.
- The reaction with positive value of Gibbs free energy are non spontaneous.
A → B ,ΔG° = -40
The value of Gibbs free energy of the reaction is negative which means that reaction is spontaneous.
