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Answer:
molality of sodium ions is 1.473 m
Explanation:
Molarity is moles of solute per litre of solution
Molality is moles of solute per kg of solvent.
The volume of solution = 1 L
The mass of solution = volume X density = 1000mL X 1.43 = 1430 grams
The mass of solute = moles X molar mass of sodium phosphate = 0.65X164
mass of solute = 106.6 grams
the mass of solvent = 1430 - 106.6 = 1323.4 grams = 1.3234 Kg
the molality =
Thus molality of sodium phosphate is 0.491 m
Each sodium phosphate of molecule will give three sodium ions.
Thus molality of sodium ions = 3 X 0.491 = 1.473 m
The enthalpy of vaporization of Bromine is 15.4 kJ/mol. -7.7 kJ is the energy change when 80.2 g of Br₂ condenses to a liquid at 59.5°C.
<h3>What is Enthalpy of Vaporization ?</h3>The amount of enthalpy or energy that must be added to a liquid substance into gas substance is called Enthalpy of Vaporization. It is also known as Latent heat of vaporization.
<h3>How to find the energy change from enthalpy of vaporization ?</h3>To calculate the energy use this expression:
where,
Q = Energy change
n = number of moles
= Molar enthalpy of vaporization
Now find the number of moles
Number of moles (n) =
=
= 0.5 mol
Now put the values in above formula we get
[Negative sign is used because Br₂ condensed here]
= - (0.5 mol × 15.4 kJ/mol)
= - 7.7 kJ
Thus from the above conclusion we can say that The enthalpy of vaporization of Bromine is 15.4 kJ/mol. -7.7 kJ is the energy change when 80.2 g of Br₂ condenses to a liquid at 59.5°C.
Learn more about the Enthalpy of Vaporization here: brainly.com/question/13776849
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Answer:
21.21°C will be the final temperature of the solution in a coffee cup calorimeter.
Explanation:
= enthalpy change = -57.2 kJ/mol of NaOH
Moles of sodium hydroxide = n
Molarity of the NaOH = 0.250 M
Volume of NaOH solution = V = 50.00 mL = 0.050 L
Moles of HCl = n'
Molarity of the HCl= 0.250 M
Volume of HCl solution = V' = 50.00 mL = 0.050 L
Since 1 mole of Hcl reacts with 1 mole of NaoH. Then 0.0125 mole of HCl will react with 0.0125 mole of NaOH.
The enthalpy change during the reaction.
q = heat released on reaction= -715 J
now, we calculate the heat gained by the solution.:
Q= -q = -(-715 J) = 715 J
m = mass of the solution = ?
Volume of the solution formed by mixing, v = 50.00 ml + 50.00 mL = 100.00 mL
Density of the solution = density of water = d = 1 g/mL
m = 100 g
q = heat gained = ?
c = specific heat =
= final temperature = ?
= initial temperature =
Now put all the given values in the above formula, we get:
21.21°C will be the final temperature of the solution in a coffee cup calorimeter.