What is the final temperature of the solution formed when 1.52 g of NaOH is added to 35.5 g of water at 20.1 °C in a calorimeter? NaOH (s) → Na+ (aq) + OH– (aq) ∆H = -44.5 kJ/mol

Answer : The final temperature of the solution in the calorimeter is,

Explanation :

First we have to calculate the heat produced.

where,

= enthalpy change = -44.5 kJ/mol

q = heat released = ?

m = mass of = 1.52 g

Molar mass of = 40 g/mol

Now put all the given values in the above formula, we get:

Now we have to calculate the final temperature of solution in the calorimeter.

where,

q = heat produced = 1.691 kJ = 1691 J

m = mass of solution = 1.52 + 35.5 = 37.02 g

c = specific heat capacity of water =

= initial temperature =

= final temperature = ?

Now put all the given values in the above formula, we get:

Thus, the final temperature of the solution in the calorimeter is,

the answer is a! (2.9 x 10^-18 j) hope i could someone. : )