Hello, folks! So, I've come across this question on my Physics homework, and I'm not entirely sure how to finish all the parts. I've included the parts I've gotten correct and what I've gone to get those answers. Use the exact values you enter in previous answer(s) to make later calculation(s). A block of copper at a temperature of 60°C is placed in contact with a block of aluminum at a temperature of 44°C in an insulated container. As a result of a transfer of 1065 J of energy from the copper to the aluminum, the final equilibrium temperature of the two blocks is 48°C. (a) What is the approximate change in the entropy of the aluminum block? (1/T) = ΔS/ΔE Plugging the numbers in, I get (1/(273+48)K) = ΔS/1065 J Solving for ΔS gave me 3.316 J/K, which was correct, according to WebAssign. (b) What is the approximate change in the entropy of the copper block? I figured it would be -3.316 J/K since the change in energy of the copper would be -1065 J and the temperature would still be 48°C since it's at equillibrium, but WebAssign seems to disagree with me. (c) What is the approximate change in the entropy of the Universe? (d) What is the change in the energy of the Universe? This one is, rather predictably, 0. Some possibly useful equations: (1/T) = ΔS/ΔE S = k*lnΩ ħ = k√(k/m) k = 1.4*10-23 J/K Ω = (q+N-1)!/(q!)(N-1)! Any help would be extremely appreciated! Thanks in advance!