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Dmitry [639]
3 years ago
13

Lithium iodide has a lattice energy of −7.3×102kJ/mol and a heat of hydration of −793kJ/mol. Find the heat of solution for lithi

um iodide. Determine how much heat is evolved or absorbed when 10.0g of lithium iodide completely dissolves in water.
Chemistry
2 answers:
Anna007 [38]3 years ago
7 0
Delta H of solution = -Lattice Energy + Hydration 
<span>Delta H of solution=- (-730)+(-793) </span>
<span>Delta H of solution= -63kJ/mol </span>

<span>Now we find moles of LiI: </span>
<span>10gLiI/133.85g=.075moles </span>
<span>multiply moles to the delta H of solution to cross cancel moles. .75moles x -64kJ/mol =4.7</span>
Maurinko [17]3 years ago
7 0

Answer:

113.6567 kiloJoules of heat is evolved or absorbed when 10.0 g of lithium iodide completely dissolves in water.

Explanation:

Lithium iodide has a lattice energy = \Delta H_{lat}=-7.3\times 10^2 kJ/mol

Lithium iodide has a heat of hydration = \Delta H_{hyd}=-793 kJ/mol

Heat of the solution of lithium iodide :

\Delta H_{soln}=\Delta H_{lat}+\Delta H_{hyd}

=-7.3\times 10^2 +(-793 kJ/mol)

= -1,523 kJ/mol

Mass of lithium iodide = 10.0g

Moles of lithium iodide = \frac{10.0 g}{134 g/mol}=0.07462 mol

Heat of the solution of lithium iodide when 0.07462 mol is dissolved: Q

Q=Moles\times \Delta H_{soln}=0.07462 mol\times (-1,523kJ/mol)

Q = -113.6567 kJ

(Negative sign indicates that energy released which means that temperature of the solution after dissolving lithium iodide  will increase.)

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