Question
Asked Feb 5, 2020
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  1. 1)  The molar enthalpy of vaporization of benzene at its boiling point (353K) i3 30.8 kJ mol-1. How much heat is needed to convert 18 g of benzene from liquid into vapors at 353 K if external pressure is 1.0 atm. What work will be done during this process?

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Expert Answer

Step 1

The number of moles of benzene is calculated as shown below where n, m, and mm are the number of moles, mass, and molar mass of the benzene respectively. The values for m and mm are substituted.

Chemistry homework question answer, step 1, image 1
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Step 2

According to the given data, 30.8 kJ of heat is required to vaporize the 1 mol or 78.11 g of liquid benzene. So, the energy required (q) to vaporize the 0.23 mol of benzene is calculated as shown below. The energy required (q) to vaporize the 0.23 mol of benzene is 7.08 kJ.Chemistry homework question answer, step 2, image 1

Chemistry homework question answer, step 2, image 2
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Step 3

The heat of 7.08 kJ is used by the system to increase the internal energy of the system and do some mechanical work due...

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