Question

Calculate ΔH° for the combustion of methane (products are
CO_{2}(g) and H_{2}O(l)), given the following
thermochemical equations:

CH4(g) + O2(g) →CH2O(g) + H2O(g) ΔH = -284 kJ

CH2O(g) + O2(g) →CO2(g) + H2O(g) ΔH = -518 kJ

H2O(g) →H2O(l) ΔH = +44 kJ

Answer #1

Calculate the ΔH∘ for this reaction using the following
thermochemical data:
CH4(g)+2O2(g)⟶CO2(g)+2H2O(l)
ΔH∘=−890.3kJ
C2H4(g)+H2(g)⟶C2H6(g)
ΔH∘=−136.3kJ
2H2(g)+O2(g)⟶2H2O(l)
ΔH∘=−571.6kJ
2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(l)

Given the following thermochemical data:
½H2(g)+AgNO3(aq) → Ag(s)+HNO3(aq) ΔH = -105.0 kJ
2AgNO3(aq)+H2O(l) → 2HNO3(aq)+Ag2O(s) ΔH = 44.8 kJ
H2O(l) → H2(g)+½O2(g) ΔH = 285.8 kJ
Use Hess’s Law to determine ΔH for the reaction:
Ag2O(s) → 2Ag(s)+½O2(g)

the combustion of methane, CH4, in oxygen.
CH4(g) + 2O2(g) >> CO2(g) + 2H2O (l)
the heat of reaction at 77C and 1.00 atm is -885.5 kJ. what is
the change in volume when 1.00 mol CH4 reacts with 2.00 mol O2.
what is w for this change?
calculate delta U (change in U) for the change indicated by the
chemical equation

Given the following data:
H2(g) + 1/2O2(g) → H2O(l)
ΔH° = -286.0 kJ
C(s) + O2(g) → CO2(g)
ΔH° = -394.0 kJ
2CO2(g) + H2O(l) →
C2H2(g) + 5/2O2(g)
ΔH° = 1300.0 kJ
Calculate ΔH° for the reaction:
2C(s) + H2(g) → C2H2(g)

Calculate the deltaH rxn for the production of CO2 and H20 via
propane combustion, using thermochemical equations below. Show all
work! 3 C (s) + 4 H2 (g) = C3H8 (g) Delta H = (-) 103.9 kJ/mol C
(s) + O2 (g) = CO2 (g) Delta H = (-) 393.5 kJ/mol H2 (g) + 1/2 O2
(g) = H2O (g) Delta H = (-)241. 8 kJ/mol Delta H rxn : ?

Octane (C8H18) undergoes combustion according to the following
thermochemical equation:
2C8H18(l) + 25O2(g) 16CO2(g) +
18H2O(l) ∆H°rxn = −10,800
kJ/mol
Given that ∆H°f[CO2(g)] = −394 kJ/mol and ∆H°f[H2O(l)] = −286
kJ/mol, calculate the standard enthalpy of formation of
octane.
a. −326 kJ/mol
b.326 kJ/mol
c.210 kJ/mol
d.-218 kJ/mol

Energy change is measured:
CH4(g) + 2 O2 (g) --> CO2 (g) + 2 H2O (l)
ΔH−882.kJ
Is the reaction endothermic or exothermic?
If 22.8g of CH4 react, will any heat be absorbed or relased?
If yes, calculate how much heat will be released or absorbed
with correct significant digits.

Thermochemical Equations 07a (kJ)
Consider the following thermochemical equation for the
combustion of butane.
2C4H10(g)+15O2(g)→8CO2(g)+10H2O(g)ΔH∘rxn=−5314.6kJ
Part A
Calculate the heat associated with the consumption of 1.158 mol
of O2 in this reaction.
Use the correct sign for q
q =
+
kJ
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Part B
Calculate the heat associated with combustion of 29.46 g of
butane.
Use the correct sign for q
q =
kJ
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Part C
Calculate the...

The thermochemical equation for the combustion of one mole of
carbon monoxide is as follows: CO(g) + ½ O2 → CO2(g) ΔH = −283 kJ
Calculate the heat change for the decomposition of 2.00 lb carbon
dioxide gas into CO and oxygen.

Hess's Law Given the following data: 2C(s) + 2H2(g) + O2(g) →
CH3OCHO(l) ΔH°=-366.0 kJ CH3OH(l) + O2(g) → HCOOH(l) + H2O(l)
ΔH°=-473.0 kJ C(s) + 2H2(g) + 1/2O2(g) → CH3OH(l) ΔH°=-238.0 kJ
H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ calculate ΔH° for the
reaction: HCOOH(l) + CH3OH(l) → CH3OCHO(l) + H2O(l)

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