Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 5.96 kcal/mol) was used in household refrigerators. what mass (in kg) of so2 must be evaporated to remove as much heat as evaporation of 1.24 kg of ccl2f2 (enthalpy of vaporization is 20.1 kj/mol)?

0.5286 kilogram of sulfur dioxide must be evaporated .

Explanation:

Enthalpy of vaporization of chlorofluorocarbons = 20.1 kJ/mol

Mass of chlorofluorocarbons  = 1.24 kg = 1240 g

Moles of chlorofluorocarbons =

Heat removes by 10.2479  moles of chlorofluorocarbons : q

Let moles  of sulfur dioxide removing 205.983 kJ(q) of heat be n.

Enthalpy of vaporization of sulfur dioxide

(1 kcal = 4.184 kJ)

n = 8.2603 moles

Mass of 8.2603 moles of sulfur dioxide =

0.5286 kilogram of sulfur dioxide must be evaporated .

the temperature of the gas, in k, not celsius.

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer