Achieve Week 3 and 4 question 10

[ElizabethTopalian 2K]

An ice cube with a mass of 46.2 g at 0.0 ∘C is added to a glass containing 3.90×102 g of water at 45.0 ∘C. Determine the final temperature of the system at equilibrium. The specific heat capacity of water, Cs, is 4.184 J/g⋅∘C, and the standard enthalpy of fusion, ΔH∘fus, of water is 6.01×103 J/mol. Assume that no energy is transferred to or from the surroundings

could someone help with this

[Ann_Ding_1J]

My numbers are slightly different, but I have attached a screenshot of my work for #10 on the Achieve. As I was reattempting the problem, I found that my biggest error was finding the heat required to melt the ice. The standard enthalpy of fusion was given, so you need to find the moles of ice and convert that value to the enthalpy of fusion in the specific reaction. From there, I used the heat equation: qp = n*Cs*ΔT. Also remember to make the water side of the equation negative because it is releasing energy. Let me know if you have any questions about my work. Hope that helps!