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When a 1.0560 g benzoic acid sample was burned in a bomb calorimeter to establish the calorimeter constant, a temperature rise of 2.862 K was measured near 298K. Under similar conditions, a temperature rise of 2.416 K was measured when a 0.5863 g naphthalene sample was burned. Determine the calorimeter constant (in units of kJ/K) and the standard enthalpy of combustion for naphthalene at 298K. If we make the assumption that ∆H ≈∆U, is the ∆cHº value obtained from this experim

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Answer:

[tex]C_{calorimeter}=7.14x10^{-4}kJ/K[/tex]

ΔcH[tex]=-337.14J/mol[/tex]

Explanation:

Hello,

In this case, naphthalene has a Cp=156.1J/(mol*K) and the following equation must be applied to find the enthalpy of combustion (negative since it is about an outgoing form of energy) considering the given assumption (∆H ≈∆U)

ΔcH=Cp*ΔT

ΔcH[tex]=156.1*2.416K\\=-337.14J/mol[/tex]

For the calorimeter constant, we develop:

[tex]C_{calorimeter}=0.5863gC_{10}H_8*\frac{1molC_{10}H_8}{128.17gC_{10}H_8} *156.1\frac{J}{mol*K}\\\\C_{calorimeter}=0.714J/K=7.14x10^{-4}kJ/K[/tex]

Best regards.

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