What is the delta H when 72.0 grams H2O condenses at 100.00C? Here are some constants that you MAY need.

specific heats heat of fusion heat of vaporization

H2O(s) = 2.1 J/g0C 6.01 kJ/mole 40.7 kJ/mole

H2O(L) = 4.18 J/g0C

H2O(g) = 1.7 J/g0C

2930 kJ

163 kJ

-163 kJ

-2930 kJ

The value of is -163 kJZ

Explanation:

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

......(1)

We are given:

Given mass of water = 72.0 g

Molar mass of water = 18 g/mol

Putting values in equation 1, we get:

Calculating the heat released for the condensation process:

......(2)

where,

= amount of heat released

n = number of moles of water = 4 moles

= specific heat of vaporization = -40.7 kJ/mol

Negative sign represents the amount of heat released.

Putting values in equation 2:

Hence, the value of is -163 kJ