Molality is one way of expressing concentration for solutions. It has units of moles of solute per kg of solvent. From the given values, we easily calculate for the moles of solute by multiplying the mass of solvent to the molality. We do as follows:
moles solute = 0.3 (10) = 3 mol solute
Smaller than; less of it will dissolve before the solution is saturated
<span>The </span>ΔH value is -22kcal
To answer this question, you need to know the Avogadro number. To find the amount of sugar molecule from mol unit you need to multiply it by the Avogadro number.
The calculation should be like this: <span>0.734 mol * 6.02*10^23 molecule/ mol= 4.41 * 10^23 molecule</span>
Answer : The amount of heat released, 45.89 KJ
Solution :
Process involved in the calculation of heat released :
Now we have to calculate the amount of heat released.
![Q=[m\times c_{p,l}\times (T_{final}-T_{initial})]+\Delta H_{fusion}+[m\times c_{p,s}\times (T_{final}-T_{initial})]](https://tex.z-dn.net/?f=Q%3D%5Bm%5Ctimes%20c_%7Bp%2Cl%7D%5Ctimes%20%28T_%7Bfinal%7D-T_%7Binitial%7D%29%5D%2B%5CDelta%20H_%7Bfusion%7D%2B%5Bm%5Ctimes%20c_%7Bp%2Cs%7D%5Ctimes%20%28T_%7Bfinal%7D-T_%7Binitial%7D%29%5D)
where,
Q = amount of heat released = ?
m = mass of water = 27 g
= specific heat of liquid water = 4.184 J/gk
= specific heat of solid water = 2.093 J/gk
= enthalpy change for fusion = 40.7 KJ/mole = 40700 J/mole
conversion : 
Now put all the given values in the above expression, we get
![Q=[27g\times 4.184J/gK\times (314-273)k]+40700J+[27g\times 2.093J/gK\times (273-263)k]](https://tex.z-dn.net/?f=Q%3D%5B27g%5Ctimes%204.184J%2FgK%5Ctimes%20%28314-273%29k%5D%2B40700J%2B%5B27g%5Ctimes%202.093J%2FgK%5Ctimes%20%28273-263%29k%5D)
(1 KJ = 1000 J)
Therefore, the amount of heat released, 45.89 KJ
