Using the provided table and the equation below, determine the heat of formation for CuBr2. CuCl2(s) + Br2(I) → CuBr2 (s) + CI2(g) ΔH = 64.1 kJ/mol
CuCl2(s) + Br2(l) CuBr2(s) + Cl2(g). ∆H= 64.1kJ/mol
Enthalpy of formation of Cl2(g) and Br2(l) are zero. I have taken values from the standard text since the values are not given in table .
∆H = enthalpy of formation of products - enthalpy of formation of reactants
64.1kJ/mol = 0 + ∆Hf,CuBr2 - ( 0 + (-205.9kJ/mol))
∆H°f, CuBr2 = 64.1 - 205.9
= - 141.8 kJ/mol. (Answer)
Using the provided table and the equation below, determine the heat of formation for CuBr2
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Question 12 of 20 Using the provided table and the equation below, determine the heat of formation for KClO2. 2 KClO2 (s) 2 KClO2 (s) + O2 (g) AH° = 296.2 kJ/mol Question 12 of 20 KCIO3 (s) -391.2 02 (9)
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