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.

each chemical family is represented as a group or column on the periodic table. based on chemical properties, there are 6 types of chemical families. group 1 represents alkali metals, group 2 represents alkaline earth metals, groups 3 to 12 represent transition metals, groups 13 to 16 represent non-metals and other metals, group 17 represents halogens and group 18 represents noble gases.