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The reaction of coal with water at high temperatures produces synthesis gas, which is a mixture of carbon monoxide and hydrogen. Use the bond energies in the table below to estimate the enthalpy of the reaction C(g) + H2O(g) ? CO(g) + H2(g) Energy(kj/mol) c-o = 358 c=o = 770 c-triple bond-o = 1070 o-h = 465 h-h = 435

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Irving Heathcote
Irving HeathcoteLv2
17 Dec 2019

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Related questions

The oxidation of hydroquinone by hydrogen peroxide in an aqueousenvironment produces quinone and water: C6H4(OH)2(aq) + H2O2(aq)-> C6H4O2(aq) + 2H2O(l) Other related reactions and theircorresponding reaction enthalpies are:

1. C6H4(OH)2(aq) -> C6H4O2(aq) + H2(g)

2. H2(g) + O2(g) -> H2O2(aq)

3. H2(g) + (1/2)O2(g) -> H2O(g)

4. H2O(g) -> H2O(l)

1. ΝH = 177.4 kJ/mol
2. ΝH = -191.2 kJ/mol

3. ΝH = -241.8 kJ/mol

4. ΝH = -43.8 kJ/mol

1. (a) What is the enthalpy change of reaction of the oxidationof hydroquinone by hydrogen peroxide in an aqueous environment, asgiven above? 1. (b) Is the oxidation reaction of hydroquinone byhydrogen peroxide endothermic or exothermic? Briefly justify youranswer in one or two sentences by referring to Νqp of the reaction.-2- 1. (c) What is the standard molar enthalpy of formation ofH2O2(aq)? What is the standard molar enthalpy of formation ofH2O(l)? 1. (d) The enthalpy of an O=O bond is 499 kJ/mol. Using theinformation given, estimate the bond enthalpy of the O-O bond inH2O2(aq). The bonds in H2O2 are: H-O-O-H.

The table below lists the average bond energies that you would need to determine reaction enthalpies.

Bond Bond energy (kJ/mol) Bond Bond energy (kJ/mol)
C−C 347 C−H 414
H−H 436 C−O 360
N=N 418 N−H 389
N≡N 946 O−H 464
O=O 498 C=O 799*

* Bond energy in CO2.

Use bond energies to calculate the enthalpy of combustion of one mole of methanol in kJ per mole methanol.

Express your answer in kilojoules as an integer.

Use bond energies to calculate ΔHrxn for the following reaction:

N2(g)+3H2(g)→2NH3(g)

Express your answer in kilojoules as an integer.

The reaction of coal and water at a high temperature produces a mixture of hydrogen and carbon monoxide gases. This mixture is known as synthesis gas (or syngas). What mass of water is required for the formation of 175 grams of carbon monoxide? C(s) + H2O(g)

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