Use Table 5.2 on slide 15 of the accompanying PowerPoint and calculate the energ

Question

Use Table 5.2 on slide 15 of the accompanying PowerPoint and calculate the energy required to combust 1 mole of ethanol and 1 mole of H_2. Assume there is one mole of ethanol for live first equation and one mole of H_2 for the second equation. In order to figure this out, follow the example calculation as on slides 14-17 for each reaction using the bond energies in Table 5.2. You will need to draw the Lewis structure for each molecule because some of the bonds are double bonds. If that is the case, watch out and use live correct bond energy in table provided. Your answer should be in kJ/mol (since you are dividing by 1 mol of the substance reacted). Ethanol: is C_2H_5OH C_2H_5OH + O_2 rightarrow CO_2 + H_2O(l) net energy change = ? kJ Balance the reaction first! H_2 + 1/2 O_2 rightarrow H_2O net energy change = ? kJ Calculate the net energy change for each reaction in slide 19. Report your answer in kJ/g and show your work? C_2H_5OJ + O_2 rightarrow CO_2 + H_2O(l) unbalanced net energy change = ? kJ/g H_2 + 1/2 O_2 rightarrow H_2O net energy change = ? kJ/g

Explanation / Answer

Q1

a)

C2H5OH + 7/2O2 = 2CO2 + 3H2O

Hrxn = Hproducts - Hreactants

HRxn = (2*-393.5 + 3*-241.818) - (-277.6 + 7/2*0)

HRxn = -1234.854kJ/mol

b)

H2 + 1/2O2 = H2O

HRxn = H2O -(H2 + 1/2O2)

HRxn = -241.818 - (0 +1/2*0)

HRxn = -241.818 kJ/mol

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