How much heat is released upon converting one mole of steam (18.0 g) from 100.0 ∘c to water at 25.0 ∘c? show work and constants, trying to figure out how it works. only given the heat capacity for steam and water so try to only use that

46418.4 Joules

Explanation:

The conversions involved in this process are :

Now we have to calculate the enthalpy change.

where,

Q = amount of heat released = ?

m = mass of water = 18 g

= specific heat of liquid water =

= enthalpy change = ?

m = mass of water = 25 g

= enthalpy change for condensation = 2265 J/g

Now put all the given values in the above expression, we get

Therefore, the amount of heat released is 46418.4 J.

c. heat could easily travel through the molecules in the air and escape/enter the flask. removing the air slows down the heat transfer.