ThermochemistryHard

Question

In an ice calorimeter, a chemical reaction is allowed to occur in thermal contact with an ice water mixture at 0oC. Any heat liberated by the reaction is used to melt some ice and the volume change of the ice water mixture indicates the amount of melting. When solutions containing 1.0 millimole each of AgNO3 and NaCl were mixed in such a calorimeter, both solutions having been pre-cooled to 0oC, 0.20 g of ice melted. Assuming complete reaction in this experiment, what is ΔH for the reaction Ag+ (aq) + Cl− (aq) → AgCl(s)?

Latent heat of fusion of ice at 0oC is 80 cal/g.

Options

A.–16 kcal
B.+16 kcal
C.−16 cal
D.+16 cal

Solution

Heat released by reaction = Heat gained by ice

$= m.L = 0.2 \times 80 = 16\text{ cal} $$$\Delta H = - \frac{16}{10^{- 3}} = - 16 \times 10^{3}\text{ cal}$$

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