How many kJ of heat energy would be absorbed when 175.0g of ethanol, C2H5OH, vaporizes at its boiling point, given the enthalpy of vaporization of ethanol is 39.3
kJ/mol?

We want the enthalpy associated with the reaction

Explanation:

H

3

CCH

2

OH

(

l

)

+

Δ

→

H

3

CCH

2

OH

(

g

)

You have a mass of

50.0

⋅

g

EtOH

, that is assumed to be at

78.3

∘

C

, and the enthalpy of vaporization is calculated by the product:

Δ

H

∘

vaporization

=

50.0

⋅

g

46.07

⋅

g

⋅

m

o

l

−

1

×

38.6

⋅

k

J

⋅

m

o

l

−

1

=

Explanation:

answer

i think the answer is a) as air pressure in an area increases, the density of the gas particles in that area decreases.

hope it