Question

8. Use the equations above for reactions 1 & 2 (and their experimental class average molar ?Hrxn values from Ques. 5), the hydrogen/oxygen equation (and its ?H) given in the Introduction, and Hess's Law to calculate the molar ?Hrxn for the combustion of Mg: Mg(s) + 1/2 O2(g) ? MgO(s) ?Hrxn = ? Show your work. ?Hf (product) = HMgO(s) = -601.2 kJ/mol ?Hf (reactant) = HMg + 1/2 HO2 0+0 = 0 ?Hrxn = (-601.2 - 0) = -601.2 kJ/mol

          8. Use the equations above for reactions 1 & 2 (and their experimental class average molar ?Hrxn values from Ques. 5), the hydrogen/oxygen equation (and its ?H) given in the Introduction, and Hess's Law to calculate the molar ?Hrxn for the combustion of Mg:
Mg(s) + 1/2 O2(g) ? MgO(s) ?Hrxn = ? Show your work.
?Hf (product) = HMgO(s) = -601.2 kJ/mol
?Hf (reactant) = HMg + 1/2 HO2 0+0 = 0
?Hrxn = (-601.2 - 0) = -601.2 kJ/mol

8. Use the equations above for reactions 1 2 (and their experimental class average molar ?Hrxn values from Ques. 5), the hydrogen/oxygen equation (and its ?H) given in the Introduction, and Hess's Law to calculate the molar ?Hrxn for the combustion of Mg:
Mg(s) + 1/2 O2(g) ? MgO(s) ?Hrxn = ? Show your work.
?Hf (product) = HMgO(s) = -601.2 kJ/mol
?Hf (reactant) = HMg + 1/2 HO2 0+0 = 0
?Hrxn = (-601.2 - 0) = -601.2 kJ/mol

Added by Jonathan M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adedamola Opalade

03/17/2022

Step 1

In this step, we will calculate the theoretical molar H value for the combustion of magnesium. Show more…

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Using the H0f values: Mg(s) = 0 kJ/mol; O2(g) = 0 kJ/mol; MgO(s) = 601.2 kJ/mol, show the calculation of the "true" (theoretical) molar H value for the reaction: Mg(s) + 1/2 O2(g) → MgO(s).