Question

Libr (s) → li (aq) br- (aq) δh = -48. 8 kj/mol in a coffee-cup calorimeter you dissolve 21. 4 g of this salt in 111 g of water at 25. 1 oc. what will be the final temperature of the solution formed?

Answer 1

Final temperature of the solution formed is 50.93ºC

As we know,

heat = mass x specific heat x change in temperature

q = mC∆T

where, m = 111 g water

             C = 4.184 J/g/deg

             ∆T = ?

To find heat we need to first find moles Libr used in this reaction:

21.4 g Libr x 1 mole/86.84 g = 0.246 moles

Therefore,

q = 0.246 moles x (-48.8) kJ/mol = -12.00 kJ = -12000 J (since it is negative, this indicates an exothermic reaction, so temperature of solution will increase).

-12000 J = (111g)(4.184 J/g/deg)(∆T)

∆T = -25.83 degrees

Final temperature = 25.1º - (-25.83º) = 50.93ºC

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