Question

3. When 3.365 g of ethanol (C$_2$H$_5$OH(l)) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is 99.472 kJ. (a) Calculate $\Delta H^\circ_{combustion}$ for ethanol at 298.15 K. (b) Calculate $\Delta H^\circ_f$ of ethanol at 298.15 K. (You will need to use some thermodynamic data from your book to answer this question).

          3. When 3.365 g of ethanol (C$_2$H$_5$OH(l)) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is
99.472 kJ.
(a) Calculate $\Delta H^\circ_{combustion}$ for ethanol at 298.15 K.
(b) Calculate $\Delta H^\circ_f$ of ethanol at 298.15 K. (You will need to use some thermodynamic data from your book to
answer this question).

3. When 3.365 g of ethanol (C2H5OH(l)) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is
99.472 kJ.
(a) Calculate Δ H^∘combustion for ethanol at 298.15 K.
(b) Calculate Δ H^ of ethanol at 298.15 K. (You will need to use some thermodynamic data from your book to
answer this question).

Added by Tony L.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

07/09/2022

Step 1

To calculate the moles of ethanol burned, we need to use the molar mass of ethanol (CH3OH). The molar mass of ethanol is calculated by adding up the atomic masses of each element in the compound. The atomic masses are: C: 12.01 g/mol H: 1.01 g/mol O: 16.00 Show more…

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3. When 3.365g of ethanol (CH3OH) is burned completely in a bomb calorimeter at 298.15 K, the heat produced is 99.472 kJ. (a) Calculate ΔHcombustion for ethanol at 298.15 K. (b) Calculate ΔHof ethanol at 298.15 K. You will need to use some thermodynamic data from your book to answer this question.