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Chapter 5: Q5.3-52E (page 271)

Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00 kcal/mol) was used in household refrigerators. What mass of \({\bf{S}}{{\bf{O}}_{\bf{2}}}\)must be evaporated to remove as much heat as evaporation of 1.00 kg of \({\bf{CC}}{{\bf{l}}_{\bf{2}}}{{\bf{F}}_{\bf{2}}}\) (enthalpy of vaporization is 17.4 kJ/mol)?

The vaporization reactions for \({\bf{S}}{{\bf{O}}_{\bf{2}}}\)and \({\bf{CC}}{{\bf{l}}_{\bf{2}}}{{\bf{F}}_{\bf{2}}}\)are\({\bf{S}}{{\bf{O}}_{\bf{2}}}{\bf{(l)}} \to {\bf{S}}{{\bf{O}}_{\bf{2}}}{\bf{(g) and CC}}{{\bf{l}}_{\bf{2}}}{\bf{F(l) }} \to {\bf{CC}}{{\bf{l}}_{\bf{2}}}{{\bf{F}}_{\bf{2}}}{\bf{(g)}}\), respectively.

Short Answer

Expert verified

The amount of SO2required is 366.848g.

Step by step solution

01

Total heat required

Here, we have to find out the amount of sulfur dioxide. To do so, we have to calculate the heat of vaporization for \(CC{l_2}{F_2}\).We already have the information on enthalpy of vaporization of \(CC{l_2}{F_2}\)and the amount of \(CC{l_2}{F_2}\).

First, we have to calculate the no of moles of \(CC{l_2}{F_2}\)and then, the amount of heat of vaporization.

\(\begin{array}{l}{\rm{Enthalpy of vaporization of CC}}{{\rm{l}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}{\rm{ = 17}}{\rm{.4 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\\{\rm{It means, the amount of heat required for vaporization of 1 mol of CC}}{{\rm{l}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}{\rm{ is 17}}{\rm{.4 kJ}}{\rm{.}}\\{\rm{Now, we have to calculate no of moles of CC}}{{\rm{l}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}{\rm{ in 1}}{\rm{.00 kg of CC}}{{\rm{l}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}\\\\{\rm{No}}{\rm{. of moles of CC}}{{\rm{l}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}{\rm{ = }}\frac{{{\rm{Weight of CC}}{{\rm{l}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}{\rm{ = 1000g}}}}{{{\rm{Molecular mass of CC}}{{\rm{l}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}{\rm{ = 121g}}}}{\rm{ = 8}}{\rm{.27 mol}}\\{\rm{Total heat required = No of moles \times Enthalpy of Vaporization}}\\{\rm{ = 8}}{\rm{.27 \times 17}}{\rm{.4 kJ }}\\{\rm{ = 143}}{\rm{.898 kJ}}\end{array}\)

02

Mass of sulphur dioxide

Now, to calculate the mass of sulfur dioxide, we need to use the information given in the question, the enthalpy of vaporization of sulfur dioxide, and the amount of heat previously calculated.

\(\begin{array}{l}{\rm{Enthalpy of vaporization of S}}{{\rm{O}}_{\rm{2}}}{\rm{ = 6 Kcalmo}}{{\rm{l}}^{{\rm{ - 1}}}}\\{\rm{It means, to vaporize 1 mol of S}}{{\rm{O}}_{\rm{2}}}{\rm{,6 Kcal energy is needed}}\\{\rm{ = 6 \times 4}}{\rm{.184 kJ energy}}\\\left[ {{\rm{1 Kcal = 4}}{\rm{.184 kJ, we are going to calculate energy in joule unit only}}} \right]\\{\rm{Now, Total heat required for CC}}{{\rm{l}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}{\rm{ is 143}}{\rm{.898 kJ}}{\rm{.}}\\{\rm{So, }}{\bf{no}}{\bf{. of moles of S}}{{\bf{O}}_{\bf{2}}}{\bf{ required = }}\frac{{{\bf{Total heat required for CC}}{{\bf{l}}_{\bf{2}}}{{\bf{F}}_{\bf{2}}}{\bf{ = 143}}{\bf{.898 kJ}}}}{{{\bf{Enthalpy of vaporization of S}}{{\bf{O}}_{\bf{2}}}{\bf{ = 6 \times 4}}{\bf{.184kJmo}}{{\bf{l}}^{{\bf{ - 1}}}}}}\\{\rm{ = 5}}{\rm{.7320 mol}}\\{\bf{Mass of S}}{{\bf{O}}_{\bf{2}}}{\bf{ = No}}{\bf{. of moles \times Molar mass of S}}{{\bf{O}}_{\bf{2}}}\\{\rm{ = 5}}{\rm{.7320 mol \times 64 gmo}}{{\rm{l}}^{{\rm{ - 1}}}}\\{\rm{ = 366}}{\rm{.848 g}}\end{array}\)

Hence, the amount of \(S{O_2}\)required is \({\rm{366}}{\rm{.848 g}}\).

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Most popular questions from this chapter

Propane, \({{\bf{C}}_{\bf{3}}}{{\bf{H}}_{\bf{8}}}\), is a hydrocarbon that is commonly used as a fuel.

(a) Write a balanced equation for the complete combustion of propane gas.

(b) Calculate the volume of air at 25 掳C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 21.0 percent O2 by volume. (Hint: we will see how to do this calculation in a later

chapter on gases鈥攆or now use the information that 1.00 L of air at 25 掳C and 1.00 atm contains 0.275 g of O2 per liter.)

(c) The heat of combustion of propane is 鈭�2,219.2 kJ/mol. Calculate the heat of formation,螖Hf 掳of propane given that螖Hf 掳of H2O(l) = 鈭�285.8 kJ/mol and螖Hf 掳of CO2(g) = 鈭�393.5 kJ/mol.

(d) Assuming that all of the heat released in burning 25.0 grams of propane is transferred to 4.00 kilograms of water, calculate the increase in temperature of the water.

If a reaction produces 1.506 kJ of heat, which is trapped in 30.0 g of water initially at 26.5 掳C in a calorimeter like that in Figure 5.12, what is the resulting temperature of the water?

Using the data in the check your learning section of example 5.5, calculate 鈭咹 in kJ/mol of AgNO3(aq) in the reaction :

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Calculate the enthalpy of combustion of propane, C3H8(g), for the formation of H2O(g) and CO2(g). The enthalpy of formation of propane is -104 kJ/mol.

A 248-g piece of copper initially at 314 掳C is dropped into 390 mL of water initially at 22.6 掳C. Assuming that all heat transfer occurs between copper and water, calculate the final temperature.
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