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Chapter 5: QCYL (page 255)

When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of \({\bf{FeC}}{{\bf{l}}_{\bf{2}}}\)(s) and 8.60 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of \({\bf{FeC}}{{\bf{l}}_{\bf{2}}}\)(s) is produced?

Short Answer

Expert verified

Enthalpy change = - 344kJ for 1 mol of \({\rm{FeC}}{{\rm{l}}_{\rm{2}}}\).

Step by step solution

01

Number of moles

The reaction is:

\({\rm{2Fe}}\left( {\rm{s}} \right){\rm{ + 2C}}{{\rm{l}}_{\rm{2}}}\left( {\rm{g}} \right) \to {\rm{FeC}}{{\rm{l}}_{\rm{2}}}\left( {\rm{s}} \right)\)

The number of moles is evaluated as:

\({\bf{Number of moles = }}\frac{{{\bf{Given mass}}}}{{{\bf{Molar mass}}}}\)

We have

\(\frac{{{\rm{1}}{\rm{.42g}}}}{{{\rm{55}}{\rm{.8g/mol}}}}{\rm{ \times 2 = 0}}{\rm{.04 mol of iron is available}}\)

\(\frac{{{\rm{3}}{\rm{.22g}}}}{{{\rm{126}}{\rm{.75g/mol}}}}{\rm{ \times 2 = 0}}{\rm{.05 mol of FeC}}{{\rm{l}}_{\rm{2}}}{\rm{ is available}}\)

02

Calculation of enthalpy change

The reaction uses 2 moles of \({\rm{FeC}}{{\rm{l}}_{\rm{2}}}\)and the conversion factor is - 8.60 / 0.05 mol of \({\rm{FeC}}{{\rm{l}}_{\rm{2}}}\). So we have,

\(\begin{array}{l}{\rm{ = }}\frac{{{\rm{ - 2 moles of FeC}}{{\rm{l}}_{\rm{2}}}{\rm{\;}} \times {\rm{8}}{\rm{.60}}}}{{{\rm{0}}{\rm{.05 FeC}}{{\rm{l}}_{\rm{2}}}{\rm{\;}}}}\\{\rm{ = - 344 kJ}}\end{array}\)

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Most popular questions from this chapter

When 1.0g of fructose, C6H12O6(s), a sugar commonly found in fruits, is burned in oxygen in a bomb calorimeter, the temperature of the calorimeter increases by 1.58藲C. If the heat capacity of the contents is 9.90kJ/藲C, what is q for this combustion?

The reaction of 50ml of acid and 50ml of base described in example 5.5 increased the temperature of the solution by 6.9 degrees. How much would the temperature have increased if 100ml of acid and 100ml base had been used in the same calorimeter starting at the same temperature of 22藲C? Explain your answer.

The decomposition of hydrogen peroxide, \({{\bf{H}}_{\bf{2}}}{{\bf{O}}_{\bf{2}}}\), has been used to provide thrust in the control jets of various space vehicles. Using the data in Appendix G, determine how much heat is produced by the decomposition of exactly 1 mole of \({{\bf{H}}_{\bf{2}}}{{\bf{O}}_{\bf{2}}}\)under standard conditions.

\({\bf{2}}{{\bf{H}}_{\bf{2}}}{{\bf{O}}_{\bf{2}}}\left( {\bf{l}} \right) \to {\bf{2}}{{\bf{H}}_{\bf{2}}}{\bf{O}}\left( {\bf{g}} \right){\bf{ + }}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right)\)

When a 3.00-g sample of KCl was added to 3.00脳102 g of water in a coffee cup calorimeter, the temperature decreased by 1.05 掳C. How much heat is involved in the dissolution of the KCl? What assumptions did you make?

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.

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