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1. 18 g of LiCl(s) is dissolved in 18.0mL of water that is initially 20.0°C. a)...

1. 18 g of LiCl(s) is dissolved in 18.0mL of water that is initially 20.0°C.

a) Write the chemical equation for the dissolution of LiCl(s)

b) Calculate the molar enthalpy of dissolving LiCl(s) in water. Is this process endothermic or exothermic?

c) Calculate the amount of heat absorbed/released when 1.18 g of LiCl(s) dissolves.

d) Calculate the final temperature of the solution. You can assume the heat capacity of solution is equal to the heat capacity of water (dwater = 1g/mL, Cp(water= 4.184 J/g°C)

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Answer #1

Lithium chloride, LiCl(s) is dissolved in water. The amount of Lici() is give as 18.0 grams. The amount of water is given asMass of LiCl(s) is given as 1.18 grams. Moles of LiCl(s) is: Mass of LiCl(s) Moles of Liais), n= Moal mass of LiCl(s) 1.18 42(d) The final temperature of the solution: Q=mCAT As the density of water is 1 g/mL, the mass of water will be same as volume

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