11.82 x 1 mole / (molar mass)
The molar mass = 197 g/mol
11.82 / 197 = .06
According to this formula when:
ΔG = ΔH - TΔS = 0
∴ ΔS = ΔH/T
∴ ΔS = n*ΔHVap / Tvap
- when n is the number of moles = mass/molar mass
when the mass = 24.1 g
and the molar mass = 187.3764 g/mol
by substitution:
∴ n = 24.1 / 187.3764g/mol
= 0.129 moles
and ΔHvap is the molar enthalpy of vaporization is 27.49 kJ/mol
and Tvap is the temperature in Kelvin = 47.6 + 273 = 320.6 K
So by substitution, we will get the ΔS the change in entropy:
∴ΔS = 0.129 mol * 27490 J/mol / 320.6 K
= 11 J/K
Answer:
As, the temperature decreased from 40.0 °C to 0.0 °C an amount will be recrystallized and precipitated as solid crystals in the water (51.0 g - 14.0 g = 37.0 g) and 14.0 g will be dissolved in water.
Explanation:
- Firstly, we must mention that:
The solubility of KNO₃ per 100.0 g of water at 40.0 °C = 63.0 g.
The solubility of KNO₃ per 100.0 g of water at 0.0 °C = 14.0 g.
- So, at 40.0 °C, 51.0 g of KNO₃ will be completely dissolved in water.
- <em>As, the temperature decreased from 40.0 °C to 0.0 °C an amount will be recrystallized and precipitated as solid crystals in the water (51.0 g - 14.0 g = 37.0 g) and 14.0 g will be dissolved in water.</em>
Answer: true
Explanation:
In chemical reactions, an energy barrier exists between reactants and products. The magnitude of this energy barrier determines the rate of reaction. A lesser energy barrier implies that reactants are converted to products faster since the energy required is not too much. On the other hand, a large energy difference between reactants and products will lead to a slow reaction with very poor yield of products if any.
Answer:
x = 100 * 1.1897 = 118.97 %, which is > 100 meaning that all of the HClO2 dissociates
Explanation:
Recall that , depression present in freezing point is calculated with the formulae = solute particles Molarity x KF
0.3473 = m * 1.86
Solving, m = 0.187 m
Moles of HClO2 = mass / molar mass = 5.85 / 68.5 = 0.0854 mol
Molality = moles / mass of water in kg = 0.0854 / 1 = 0.0854 m
Initial molality
Assuming that a % x of the solute dissociates, we have the ICE table:
HClO2 H+ + ClO2-
initial concentration: 0.0854 0 0
final concentration: 0.0854(1-x/100) 0.0854x/100 0.0854x / 100
We see that sum of molality of equilibrium mixture = freezing point molality
0.0854( 1 - x/100 + x/100 + x/100) = 0.187
2.1897 = 1 + x / 100
x = 100 * 1.1897 = 118.97 %, which is > 100 meaning that all of the HClO2 dissociates
