Question

Before the introduction of chlorofluorocarbons, sulfur dioxide (entha;py of vapourization, 6.00 kcal/mol) was used in household refrigrators. What mass of SO2 must be evoparated o remove as much heat as evaporation of 1.00 kg of CCl2F2(enthalpy of vapourization is 17.4 kJ/mol)?

The vapourition reactions for SO2 and CCl2F2 re SO2 (i) ? SO2 and CCl2F(i) ? CCl2F2(g), respectively

Answer 1

Answer: 367 grams

Step-by-step explanation:

According to avogadro's law, 1 mole of every substance weighs equal to the molecular mass and contains avogadro's number
`6.023* 10^(23)` of particles.

Enthalpy of vaporization is the amount of heat released when 1 mole of substance is converted from liquid to gaseous state.

Given : Enthalpy of vapourization of
`CCl_2F_2` = 17.4 kJ/mol

To calculate the number of moles, we use the equation:

`\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}`

`\text{Number of moles of}CCl_2F_2=(1000g)/(121g/mol)=8.3moles`

1 mole of
`CCl_2F_2` produces heat = 17.4 kJ

8.3 moles of
`CCl_2F_2` produces heat =
`(17.4)/(1)* 8.3=144 kJ`

Given : Enthalpy of vapourization of
`SO_2` = 6.0 kcal/mol =
`6* 4.184=25.104kJ` (1kcal=4.184kJ)

25.104 kJ heat is produced by = 1 mole of
`SO_2`

144 kJ heat is produced by =
`(1)/(25.104)* 144=5.73mole` of
`SO_2`

Mass of
`SO_2=moles* {\text {molar mass}}=5.73* 64=367g`

Thus 367 grams of
`SO_2` must be evoparated o remove as much heat as evaporation of 1.00 kg of
`CCl_2F_2`