# Thermochemistry Problem

haydn

## Homework Statement

When 0.612 g of Ca metal is added to 200.0 mL of 0.500 M HCl(aq), a temperature increase of 100C is observed.
Assume the solution's final volume is 200.0 mL, the density is 1.00 g/mL, and the heat capacity is 4.184 J/gC.
(Note: Pay attention to significant figures. Do not round until the final answer.)
The molar heat of reaction, H rxn, for the reaction of

Ca(s) + 2H+(aq) => Ca2+(aq) + H2 (g)

## Homework Equations

Q=mc$$\Delta$$T

## The Attempt at a Solution

All I know is that mc$$\Delta$$T is used... Our professor hasn't taught us how to do this yet so that's about all I know. Would I divide Q by the number of moles formed?