Answer
138.96$^{\circ}$C, Hg
Work Step by Step
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
