Problem

Two

100\text{ cm}^3

aqueous solutions, one containing

0.010\text{ mol NaOH}

and the other containing

0.010\text{ mol HCl}

, are at the same temperature. When the two solutions are mixed the temperature rises by

y^\circ\text{C}

. Assume the density of the final solution is

1.00\text{ g cm}^{-3}

. Specific heat capacity of water =

4.18\text{ J g}^{-1}\text{ K}^{-1}

What is the enthalpy change of neutralization in

\text{kJ mol}^{-1}

? a.

\frac{200 \times 4.18 \times y}{1000 \times 0.020}

\frac{200 \times 4.18 \times y}{1000 \times 0.010}

\frac{100 \times 4.18 \times y}{1000 \times 0.010}

\frac{200 \times 4.18 \times (y + 273)}{1000 \times 0.010}