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This would be a certain question about calorimetry.

You must first understand that heat is "energy in transition", which means it cannot be stored but it "moves" from one body to another.

Using this concept, we can then assume that no heat was lost to the surroundings.

Therefore we use the equation:

0 = Qgain + Qloss

where:

Qgain = heat gained by the insulated aluminum cup

Qloss = heat lost by the hot water (at 50°C water is relatively warm. :D)

Further continuing the solution:

we use the Q=mcΔT to measure quantities of heat involved in the problem:

where:

m = mass of object

c = specific heat constant

ΔT = change in temperature

Continuing:

0 = mcΔT + mcΔT

0 = (0.115 kg)(910 J/kg-K)(Tfinal - 15°C) + (0.143 kg)(4190 J/kg-K)(Tfinal - 50°C)

Solving for T we get:

T =44.79 C°

This is the final temperature when the system has reached equilibrium! The problem is pretty plain and simple! With a bit of practice and a lot of solving seasoned with determination, you can master temperature topics in Physics!

Keep practicing! :)