Determine the delta H degree of reaction [2]. [1]CH_4(g) + 2 O_2(g) rightarrow 2

Question

Determine the delta H degree of reaction [2]. [1]CH_4(g) + 2 O_2(g) rightarrow 2 CO_2 + H_2O delta H = -91.8 kJ [2] 4 CO_2 + 2H_2O rightarrow CH_4(g) + 4 O_2 (g) Using Hess's law, determine the delta H degree of reaction [4]. [1] 4 HCl(s) + O_2 (g) rightarrow 2 H_2O (l) + 2 Cl_2 (g) delta H = -204.2 kJ [2] H_2 (g) + F_2 (g) rightarrow 2 HF (l) delta H = -1200.0 kJ [3] 2 H_2 (g) + O_2 (g) rightarrow 2 H_2O (l) delta H = -571.6 kJ [4] 2 HCl(s) + F_2 (g) rightarrow 2 HF (l) + Cl_2 (g) When 50.00 mL of 1.00 M HCl is reacted with 0.400 g of zinc metal in a calorimeter, the temperature rises from 25.00 degree C to 32.18 degree C. Assume that the specific heat of the solution is 4.18 J/g degree C and its density is 1.00 g/mL. Calculate the molar enthalpy change in kilojoules/mole of zinc.

Explanation / Answer

1)

Given for:

CH4(g) + 2 O2(g) ---> 2 CO2 + H2O

HO1 rxn = 2*Hof(CO2) + Hof(H2O) - Hof( CH4(g)) - 2*Hof(O2(g)) = -91.8 KJ

we need to calculate for:

4 CO2 + 2 H2O ---> 2 CH4(g) + 4 O2(g)

Ho2 rxn = 2*Hof(CH4(g)) + 4*Hof(O2(g)) - 4*Hof( CO2) - 2*Hof(H2O)

Ho2 rxn = 2*[Hof(CH4(g)) + 2*Hof(O2(g)) - 2*Hof( CO2) - Hof(H2O)]

Ho2 rxn = -2*[2*Hof(CO2) + Hof(H2O) - Hof( CH4(g)) - 2*Hof(O2(g))]

Ho2 rxn = -2*[Ho1 rxn]

Ho2 rxn = -2*[-91.8 KJ]

Ho2 rxn = 183.6 KJ

Answer: 183.6 KJ

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