Calorimetry help

Question

1. A 138.6 g sample of copper is heated from 16.24°C to 204.87°C. What is the amount of heat transferred? specific heat capacity of Cu = 0.385 J/g-K a chemical equation for the reaction

2. A 52.19 mL sample of 3.02 M CuSO4 reacts with 54.48 mL of 2.87 M KOH in a coffee cup calorimeter to form Cu(OH)2(s) and K2SO4 (aq). The initial temperature is 18.5°C and the final temperature is 44.9°C. Assume that the mixture has the same specific heat as water and the same density as water. Specific heat of water is 4.184 J/g-K.

a.) Write a chemical equation for the reaction.

b.) How many moles of CuSO4 reacted?

c.) How many moles of KOH reacted?

d.) Which reactant is the limiting reagent?

e.) How much heat, in J, was transferred to the solution?

f.) How much heat, in kJ, was transferred by the reaction?

g.) Calculate the heat transferred by the reaction in kJ/ mol (use the limiting reagent moles)

h.) Is the reaction exothermic or endothermic?

Answer 1

I will answer the first question. Take note of J.R.S.' comment. On this website, you should post specific questions, one at a time.

(1)

Q = mc(T₂ - T₁)

m = 138.6 g

c = 0.385 J/(gK)

T₁ = 16.24°C

T₂ = 204.87°C

Plug in the numbers and get Q in joules. Note that the temperature difference T₂ - T₁ is the same in °C and in K.