In the following experiment, a coffee-cup calorimeter containing 100 g of H2O is used. The initial temperature of the calorimeter is 23.0 oC. If 2.8 g of CaCl2is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? Assume that the heat capacity of the solution is 4.18 J/goC, and that the heat capacity of the calorimeter is negligible. The heat of dissolution ΔHsoln of CaCl2 is −82.8 kJ/mol.

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answer: -

reaction:

na + cl ⇌ nacl

balanced chemical equation:

na + 2cl ⇌ nacl2

sodium + clorine goes to form sodium chloride (table salt).

the product is nacl2.

and the reactants are na and cl.

(note: if you don’t know what ⇌ means, read below: -

⇌(double head arrow) means reversible reaction).

the dependant variable is spilled water

the independent is the heat

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i think? ?