Question

When 50.0 mL of water containing 0.50 mol HCl at 22.5°C are mixed with 50.0 mL of water containing 0.50 mol NaOH at 22.5°C in a calorimeter, the temperature of the solution increases to 26.0°C. How much heat (in kJ) was released by this reaction? Note: the specific heat of water (Cwater) is 4.18 J/(g•˚C) and the density of the solution is 1.00 g/mL.

Answer 1

Answer:

1.46kj

Explanation:

Answer 2

The heat (in kJ)  released by this reaction is mathematically given as

Hp=-28.5kJ

What is the heat (in kJ)  released by this reaction?

Question Parameter(s):

When 50.0 mL of water containing 0.50 mol HCl at 22.5°C

mixed with 50.0 mL of water containing 0.50 mol NaOH at 22.5°C

the temperature of the solution increases to 26.0°C.

Generally, the equation for the Chemical Reaction   is mathematically given as

Hp=H_{H_2O} +H_{rxn}

Therefore,Heat of water

H_{H_2O}=[(50.0mL+50mL)*4.18*(26.0-22.5)

H_{H_2O}=146.3J

H_{H_2O}=0.1463kJ

In conclusion, Hp

Hp=-(0.1463+28.36)

Hp=-28.5kJ

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