When \(2.0 \mathrm{g}\) of \(\mathrm{NaOH}\) were dissolved in \(53.0 \mathrm{g}\)
water in a calorimeter at \(24.0^{\circ} \mathrm{C}\), the temperature of the
solution went up to \(33.7^{\circ} \mathrm{C}\).
a. Is this solution reaction exothermic? ______ Why?
b. Calculate \(q_{H_{2} o},\) using Eq. 1 _______ joules
c. Find \(\Delta H\) for the reaction as it occurred in the calorimeter (Eq. 5
). \(\Delta H=\) ________ joules
d. Find \(\Delta H\) for the solution of \(1.00 \mathrm{g} \mathrm{NaOH}\) in
water. \(\Delta H=\) _______ joules/g
e. Find \(\Delta H\) for the solution of one mole \(\mathrm{NaOH}\) in water.
\(\Delta H=\) _______ joules/mole
f. Given that NaOH exists as \(\mathrm{Na}^{+}\) and \(\mathrm{OH}^{-}\) ions in
solution, write the equation for the reaction that occurs when \(\mathrm{NaOH}\)
is dissolved in water.
g. Using cnthalpies of formation as given in thermodynamic tables, calculate
\(\Delta H\) for the reaction in Part f and compare your answer with the result
you obtained in Part e.
