A 15.0-g sample of liquid ethanol, C2 H5 OH, absorbs 5.13 ×10^3 J of heat at its normal boiling

step 1 In this problem, we're given the mass of a sample of liquid ethanol, and we're told it absorbed

A 15.0-g sample of liquid ethanol, C2 H5 OH, absorbs 5.13...

A $15.0-g$ sample of liquid ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$, absorbs $5.13 \times 10^{3} \mathrm{~J}$ of heat at its normal boiling point, $78.0^{\circ} \mathrm{C}$. The molar enthalpy of vaporization of ethanol, $\Delta H_{\text {vap, }}$, s $39.3 \mathrm{~kJ} / \mathrm{mol}$. (a) What volume of $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ vapor is produced? The volume is measured at $78.0^{\circ} \mathrm{C}$ and $1.00$ atm pressure. (b) What mass of $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ remains in the liquid state?

A $15.0-g$ sample of liquid ethanol, $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$, absorbs $5.13 \times 10^{3} \mathrm{~J}$ of heat at its normal boiling point, $78.0^{\circ} \mathrm{C}$. The molar enthalpy of vaporization of ethanol, $\Delta H_{\text {vap, }}$, s $39.3 \mathrm{~kJ} / \mathrm{mol}$. (a) What volume of $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ vapor is produced? The volume is measured at $78.0^{\circ} \mathrm{C}$ and $1.00$ atm pressure.
(b) What mass of $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ remains in the liquid state?

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Key Concepts

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, relates pressure, volume, temperature, and the number of moles of a gas. It is used to determine the volume that a given amount of vapor will occupy under specified conditions of temperature and pressure.

Heat Transfer in Phase Transitions

In phase transitions, the supplied heat does not increase the temperature but is used to overcome intermolecular forces. The concept involves determining how much of a substance undergoes a phase change based on the amount of energy provided relative to the enthalpy of vaporization.

Enthalpy of Vaporization

This concept refers to the amount of energy required to convert one mole of a substance from the liquid phase to the vapor phase at its boiling point. It is a form of latent heat and is essential in understanding the energy changes involved during phase transitions.

Molar Mass and Mole Calculations

Understanding the relationship between mass, molar mass, and the number of moles is fundamental in chemistry. It allows the conversion of a given mass of a substance into moles, which is necessary for stoichiometric calculations and applying thermodynamic quantities on a per-mole basis.

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