Question

The following reaction takes place at isothermal conditions at T = 598 K CH$_3$COOH + 2 H$_2$ \leftrightarrow C$_2$H$_5$OH + H$_2$O At 298 K, reaction enthalpy is: $\Delta H^{\circ}_{298}$ = 7580 J/mol, The average heat capacities for these compounds between T = 298 and T = 598 are: $[Cp]CH_3COOH$ = 10.6 J/mol K $[Cp]C_2H_5OH$ = 11.1 J/mol K $[Cp]H_2$ = 3.5 J/mol K $[Cp]H_2O$ = 4.2, J/mol K What is $\Delta H^{\circ}$ at 598 K? How much heating or cooling per mole reaction of would be required to keep the system at its fixed Temperature?

          The following reaction takes place at isothermal conditions at T = 598 K
CH$_3$COOH + 2 H$_2$ \leftrightarrow C$_2$H$_5$OH + H$_2$O
At 298 K, reaction enthalpy is: $\Delta H^{\circ}_{298}$ = 7580 J/mol,
The average heat capacities for these compounds between T = 298 and T = 598 are:
$[Cp]CH_3COOH$ = 10.6 J/mol K
$[Cp]C_2H_5OH$ = 11.1 J/mol K
$[Cp]H_2$ = 3.5 J/mol K
$[Cp]H_2O$ = 4.2, J/mol K
What is $\Delta H^{\circ}$ at 598 K?
How much heating or cooling per mole reaction of would be required to keep the system at its fixed
Temperature?

Show more…

The following reaction takes place at isothermal conditions at T = 598 K
CH3COOH + 2 H2 ↔C2H5OH + H2O
At 298 K, reaction enthalpy is: Δ H^∘298 = 7580 J/mol,
The average heat capacities for these compounds between T = 298 and T = 598 are:
[Cp]CH3COOH = 10.6 J/mol K
[Cp]C2H5OH = 11.1 J/mol K
[Cp]H2 = 3.5 J/mol K
[Cp]H2O = 4.2, J/mol K
What is Δ H^∘ at 598 K?
How much heating or cooling per mole reaction of would be required to keep the system at its fixed
Temperature?

Added by Nicole B.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Supreeta N

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ΔH = H'298 + ∫[Cp]dT ΔH = 7580 J/mol + ∫[Cp]dT ΔH = 7580 J/mol + ∫(10.6 J/mol K)dT + 2∫(3.5 J/mol K)dT - ∫(11.1 J/mol K)dT - ∫(4.2 J/mol K)dT ΔH = 7580 J/mol + 10.6(T - 298) + 2(3.5)(T - 298) - 11.1(T - 298) - 4.2(T - 298) ΔH = 7580 J/mol + 10.6T - 3168.8 + 7T - Show more…

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The following reaction takes place at isothermal conditions at T = 598 K: CH3COOH + 2 H2 -> CH5OH + H2O At 298 K, the reaction enthalpy is: H'298 = 7580 J/mol. The average heat capacities for these compounds between T = 298 and T = 598 are: [Cp]CH3COOH = 10.6 J/mol K [Cp]H2 = 3.5 J/mol K [Cp]C2H5OH = 11.1 J/mol K [Cp]H2O = 4.2 J/mol K What is H at 598 K? How much heating or cooling per mole of reaction would be required to keep the system at its fixed temperature?

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