A1000 ml sample of 0.300 m naoh is mixed with 100.0 ml of 0.300 m hcl in a coffee cup calorimeter. if both solutions are at 20.0 °c and the final temperature of the mixture was 22.0 °c find the heat of neutralization, ahreu in kj/mole. assume no heat is lost to the surroundings, the density of all solutions is 1.00 g/ml, and c, of the mixture is 4.184 j/g·°c

ΔH(neu) = 30.68 kJ/mol

Explanation:

The reaction between HCl (strong acid) and NaOH(strong base) is a neutralization reaction which yields sodium chloride NaCl and water

The heat (q) of a reaction is given as:

where m = mass of the system

c = specific heat

T1 and T2 are the initial and final temperatures

It is given that:

Volume of HCl = 1000 ml

Volume of NaOH = 100.0 ml

Density of HCl and NaOH = 1.000 g/ml

Total mass of the solutions, m = 1000 +100.0 = 1100.0 g

c = 4.184 J/g/c

T1 = 20.0C

T2 = 22.0 C

Substituting appropriate values in equation (1) gives:

Now, the number of moles of NaOH is:

Enthalpy of neutralization is:

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the dependant variable is spilled water

the independent is the heat