Question

When 50.0 mL of water containing 0.50 mol HCl at 22.5°C is 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) is released by this reaction? The density of water is 1.00 g/mL, and the heat capacity is 4.18 J/(g°C). (3 sig figs, kJ)

Answer 1

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Answer 2

Given:

total volume of water = 50ml+50ml = 100ml

Initial temperature = 22.5°C

final temperature = 26.0°C

density of water = 1 g/ml

heat capacity(C) = 4.18J/(g°C)

To Find:

heat (in kJ) is released by this reaction = q =?

Solution:

now, we know the expression to calculate the heat,

q = m × C × ΔT

from total volume of water = 50ml+50ml = 100ml and density of water = 1 g/ml, we can calculate mass of water as shown below.

density = mass/volume

mass = density × volume = 1 × 100 = 100g

similarly, ΔT = final temperature - initial temperature = 26 - 22.5 = 3.5°C

and heat capacity(C) = 4.18J/(g°C) is given

now, on putting values in the above equation.

q = m × C × ΔT

q = 100 × 3.5°C × 4.18 = 1463 J = 1.46 kJ

Hence, 1.46kJ heat is released by this reaction.