## Chemistry 9th Edition

138.96$^{\circ}$C, Hg
Use the equation q = mass * specific heat * $\Delta$temperature Solving for substance in table 6.1 that requires largest amount of energy to raise temp 22$^{\circ}$C (Specific heat of water = 4.18) q = 25g * 4.18 * 22$^{\circ}$C q = 2299 J, H2O Solving for substance in table 6.1 that has the largest temp chance Convert 10.7 kJ to 10700 J 10700 J = 550g * .14 * $\Delta$T 10700 J = 77 * $\Delta$T * $\Delta$T = 138.96$^{\circ}$C, Hg