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.

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"