Avolume of 500.0 ml of 0.220 m hcl(aq) was added to a high quality constant-pressure calorimeter containing 500.0 ml of 0.200 m naoh(aq). both solutions have a density of 1.000 g ml-1 and a specific heat of 4.184 j g‑1 oc-1. the temperature of the entire system rose from 25.60 °c to 26.70 °c. calculate the heat of reaction, in kj, per mole of naoh(aq).

Heat of the reaction per mole of NaOH = 46.02 kJ/mol

Explanation:

The reaction between HCl (strong acid) and NaOH(strong base) is a neutralization reaction which yields a salt 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 = 500.0 ml

Volume of NaOH = 500.0 ml

Density of HCl and NaOH = 1.000 g/ml

Total mass of the solutions, m = 500.0 +500.0 = 1000.0 g

c = 4.184 J/g/c

T1 = 25.6 C

T2 = 26.70 C

Substituting appropriate values in equation (1) gives:

Now, the number of moles of NaOH is:

Heat of reaction/mole NaOH is:

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.