I have no idea what this is about, I keep reading it over and other again, but I still don't understand! Help?
1 answer:
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Explanation:
For the given reaction, the temperature of liquid will rise from 298 K to 339 K. Hence, heat energy required will be calculated as follows.
Putting the given values into the above equation as follows.
=
= 1902.81 J
Now, conversion of liquid to vapor at the boiling point (339 K) is calculated as follows.
= energy required =
= latent heat of vaporization
Therefor, calculate the value of energy required as follows.
=
=
= 12121.2 J
Therefore, rise in temperature of vapor from 339 K to 373 K is calculated as follows.
Value of = 1.06 J/g,
= (373 -339) K = 34 K
Hence, putting the given values into the above formula as follows.
=
= 983.892 J
Therefore, net heat required will be calculated as follows.
Q =
= 1902.81 J + 12121.2 J + 983.892 J
= 15007.902 J
Thus, we can conclude that total energy (q) required to convert 27.3 g of THF at 298 K to a vapor at 373 K is 15007.902 J.