2 of 6 FINISH QUIZ O SHORT ANSWER How much energy does it take to raise 72 g of liquid ethanol at 48°C to a boil at 78°C andicompletely evaporate? Latent heat of fusion = 109 J/g Latent heat of vaporization = 838 J/g Specific Heat = 2.44 J/g*°C Enter Answer Here
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
![### Understanding the Energy Required to Heat and Evaporate Ethanol
**Question**
How much energy does it take to raise 72 g of liquid ethanol at 48°C to a boil at 78°C and completely evaporate?
**Given Data:**
- Latent heat of fusion = 109 J/g
- Latent heat of vaporization = 838 J/g
- Specific Heat = 2.44 J/g*°C
**Solution:**
1. **Calculate the energy required to heat the ethanol from 48°C to 78°C:**
\[
\text{Q} = \text{mass} \times \text{specific heat} \times \Delta \text{T}
\]
\[
\text{Q} = 72 \, \text{g} \times 2.44 \, \text{J/g*°C} \times (78°C - 48°C)
\]
\[
\text{Q} = 72 \, \text{g} \times 2.44 \, \text{J/g*°C} \times 30 \, \text{°C}
\]
\[
\text{Q} = 72 \times 2.44 \times 30 = 5270.4 \, \text{J}
\]
2. **Calculate the energy required to evaporate the ethanol:**
\[
\text{Q} = \text{mass} \times \text{latent heat of vaporization}
\]
\[
\text{Q} = 72 \, \text{g} \times 838 \, \text{J/g}
\]
\[
\text{Q} = 72 \times 838 = 60336 \, \text{J}
\]
3. **Total Energy Required:**
\[
\text{Total Energy} = \text{Energy to heat the ethanol} + \text{Energy to evaporate the ethanol}
\]
\[
\text{Total Energy} = 5270.4 \, \text{J} + 60336 \, \text{J}
\]
\[
\text{Total Energy} = 65606.4 \, \text{J}](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbff3d814-adb3-42b6-9008-5c333146b127%2F4dfb02af-b451-433d-87ea-70b8b92750d4%2Fpsfe4eq_processed.jpeg&w=3840&q=75)
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