Benzene, C6H6, is a clear colorless to light-yellow liquid, flammable with a petroleum-like, aromatic odor. Benzene is less dense than water and is slightly soluble in water.Hence it floats on water.Benzene vapor is heavier than air. Benzene causes central nervous system damage acutely and bone marrow damage chronically and is carcinogenic. The molar enthalpy of vaporization of benzene at its boiling point (3 5 3 K) is 3 0. 8 4 k J m o l − 1. What is the molar internal energy change? For how long would a 1 2 V source need to supply a 0. 5 A current in order to vaporises 7. 8 g of the sample at its boiling point? The LibreTexts libraries are Powered by MindTouch ® and are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739.

The enthalpy of vaporization of benzene C6H6(l), , is 33.9 kJ/mol at 298K .

How many liters of C6H6 (g) measured at 298K and 94.9mmHg , are formed when 1.52kJ of heat is absorbed by C6H6(l) at a constant temperature of 298K ?

The Enthalpy Of Vaporization Of Benzene Is 33.9 At 298 Divided

Can someone please work this problem step by step, it would be greatly appreciated.

The Enthalpy Of Vaporization Of Benzene Is 33.9 At 298 Inches

C6H6(l) ---> C6H6(g) DeltaH = + 33.9 kJ/mol
So if 33.9 kJ vaporise 1 mole of benzene
then 1.52 kJ will vaporise (1/33.9) x 1.52 = 0.0448 moles of benzene.
If one mole of benzene has a mass of 78g, then 0.0448 moles will have a mass of 3.497g.
If density of liquid benzene is 0.8765 g/cm3, then the volume of this will be 3.99 cm3