Question

Thermochemistry Hess's Law Reaction Equations C$_2$H$_4$O$_2$(l) + 2 O$_2$(g) $\rightarrow$ 2 CO$_2$(g) + 2 H$_2$O(g) $\Delta H^\circ_{rxn}$ = -786.3 kJ/mol H$_2$O(g) $\rightarrow$ H$_2$O(l) $\Delta H^\circ_{rxn}$ = -44.0 kJ/mol Calculate the enthalpy change ($\Delta H^\circ_{rxn}$) for the following reaction using the data in the above table. C$_2$H$_4$O$_2$(l) + 2 O$_2$(g) $\rightarrow$ 2 CO$_2$(g) + 2 H$_2$O(l) -742.3 X kJ/mol

          Thermochemistry
Hess's Law
Reaction Equations
C$_2$H$_4$O$_2$(l) + 2 O$_2$(g) $\rightarrow$ 2 CO$_2$(g) + 2 H$_2$O(g)  $\Delta H^\circ_{rxn}$ = -786.3 kJ/mol
H$_2$O(g) $\rightarrow$ H$_2$O(l)
$\Delta H^\circ_{rxn}$ = -44.0 kJ/mol
Calculate the enthalpy change ($\Delta H^\circ_{rxn}$) for the following reaction using the data in the above table.
C$_2$H$_4$O$_2$(l) + 2 O$_2$(g) $\rightarrow$ 2 CO$_2$(g) + 2 H$_2$O(l)
-742.3
X kJ/mol

Thermochemistry
Hess's Law
Reaction Equations
C2H4O2(l) + 2 O2(g) → 2 CO2(g) + 2 H2O(g) Δ H^∘rxn = -786.3 kJ/mol
H2O(g) → H2O(l)
Δ H^∘rxn = -44.0 kJ/mol
Calculate the enthalpy change (Δ H^∘rxn) for the following reaction using the data in the above table.
C2H4O2(l) + 2 O2(g) → 2 CO2(g) + 2 H2O(l)
-742.3
X kJ/mol

Added by Cheryl F.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Susan Hallstrom

06/04/2023

Step 1

Step 1: We can use Hess's Law to calculate the enthalpy change for the given reaction by manipulating the given equations to cancel out the intermediate species (H2O(g)) and add the enthalpy changes. Show more…

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Thermochemistry Hess's Law Reaction Equations C2H4O2(l) + 2O2(g) -> 2CO2(g) + 2H2O(g) ΔHrxn^0 = -786.3 kJ/mol H2O(g) -> H2O(l) ΔHrxn^0 = -44.0 kJ/mol Calculate the enthalpy change (ΔHrxn^0) for the following reaction using the data in the above table. C2H4O2(l) + 2O2(g) -> 2CO2(g) + 2H2O(l) -742.3 kJ/mol