Aquantity of 8.10 × 102 ml of 0.600 m hno3 is mixed with 8.10 × 102 ml of 0.300 m ba(oh)2 in a constant-pressure calorimeter of negligible heat capacity. the initial temperature of both solutions is the same at 18.46°c. the heat of neutralization when 1.00 mol of hno3 reacts with 0.500 mol ba(oh)2 is −56.2 kj/mol. assume that the densities and specific heats of the solution are the same as for water (1.00 g/ml and 4.184 j/g · °c, respectively). what is the final temperature of the solution?

22.48°C is the final temperature of the solution.

Explanation:

Heat of neutralization of reaction , when 1 mol of nitric acid reacts= ΔH= -56.2 kJ/mol= -56200 J/mol

Moles of nitric acid = n

Volume of nitric acid solution =

Molarity of the nitric acid = 0.600 M

Moles of barium hydroxide = n'

Volume of barium hydroxide solution =

Molarity of the barium hydroxide= 0.300 M

According to reaction, 2 mol of nitric acid reacts with 1 mol of barium hydroxide .Then 0.486 mol of nitric acid will react with :

barium hydroxide.

Heat release when 0.486 mol of nitric acid reacted = Q

= ΔH × 0.486 = -56200 J/mol × 0.486 mol=-27,313.2 J

Heat absorbed by the mixture after reaction = Q' = -Q = 27,313.2 J

Volume of the nitric solution = 0.81 L = 810 mL

Volume of the ferric nitrate solution = 0.81 L = 810 mL

Total volume of the solution = 810 mL + 810 mL = 1620 mL

Mass of the final solution = m

Density of water = density of the final solution = d = 1 g/mL

Initial temperature of the both solution were same =

Final temperature of the both solution will also be same after mixing=

Heat capacity of the mixture = c = 4.184 J/g°C

Change in temperature of the mixture = ΔT =

22.48°C is the final temperature of the solution.

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