Answer :
Answer: The answer is 62.8 kJ
Explanation: First you need to change 75.0g of c2h5oh into moles.
75.0g / 46.069g = 1.628mol
Then you need to multiply by ΔHvap
1.628mol x 38.6kJ/mol = 62.8 kJ
Final answer:
About 62.9 kilojoules (kJ) of heat are needed to evaporate 75.0g of C2H5OH. This is calculated by determining the number of moles in 75.0g and then using the heat of vaporization to find the total amount of heat.
Explanation:
To calculate the amount of heat needed to evaporate 75.0g of C2H5OH, we first determine the number of moles of C2H5OH. Using the molar mass of C2H5OH, which is approximately 46.07 g/mol, we find that there are about 1.63 moles in 75.0g.
Next, we multiply the number of moles by the heat of vaporization, which is given as 38.6 kJ/mol. The calculation is as follows: 1.63 mol x 38.6 kJ/mol = 62.9 kJ.
Therefore, about 62.9 kilojoules (kJ) of heat are required to evaporate 75.0g of C2H5OH.
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