Chemistry 30

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Thermodynamics

Assignment 3: Calculating Heats of Reaction
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1.

When iron rusts in air, the following reaction occurs:

4 Fe (s) + 3 O2 (g) → 2 Fe2O3 (s)    ΔH = -1643 kJ

What is the heat of formation, ΔHf, of Fe2O3?

(hint: what is the heat of formation reaction for Fe2O3? How does this reaction compare to the reaction given in the question?)

2.

The equation for the decomposition of mercury(II) oxide is as follows:

2 HgO (s) + 182 kJ → 2 Hg (l) + O2 (g)

Determine ΔHf for HgO (s) ?

(hint: What does ΔHf mean? What would be the overall equation associated with ΔHf ?)

3. Using a table of thermochemical data, calculate ΔH ° for the following reactions. Show your work.
  a. CO (g) + ½ O2 (g) → CO2 (g)
  b. CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (g)
  c. CS2 (g)+ 2 H2O (l) → CO2 (g) + 2 H2S (g)
4.

Calculate ΔH ° for the process:

2 Al(s) + Fe2O3 (s) → Al2O3 (s) + 2 Fe (s)

Given that ΔHf° of Fe2O3 = -813.0 kJ/mole and ΔHf° of Al2O3 is -1,655.0 kJ/mol

5.

The standard heats of formation for CH4, CHCl3 and HCl are -74.8, -132, -92.0 kJ/mole, respectively. Use this information to calculate the heat of reaction for the following reaction:

CH4 + 3 Cl2 → CHCl3 + 3 HCl

6.

The standard heat of formation, ΔHf, for C2H4 is +52.3 kJ/mol. If C2H4 (ethylene) reacts with H2 to produce C2H6 (ethane) according to the following equation:

C2H4 + H2 → C2H6   ΔH = -137 kJ

what is the heat of formation of C2H6?

(Hint : Solve this question without looking up ΔHf° for C2H6 in the Table of Thermochemical Data, although you may want to in order to check your answer. Solve this using the standard formula, ΔH reaction = ∑ ΔH products - ∑ ΔH reactants. However, this time you know ΔH reaction and need to solve for a substance on the product side of the equation.)

7.

Using bond enthalpies, calculate ΔH for the following reaction:

N2 + 2 H2 → N2H4

The structural formulas for all reaction participants are shown here:

 

N — N + 2 H — H

molecule - N2H4, hydrazine

8.

The energy from the combustion of hydrazine, N2H4 , is used to power rockets into space in the reaction:

N2H4 (g) + O2 (g) → N2 (g) + 2 H2O (l)    ΔH ° = -627.6 kJ/mol

How many kilograms of hydrazine would be necessary to produce 1.0 × 108 kJ of energy?

Hint: One mole of N2H4 produces 627.6 kJ of energy. How many moles (and then grams) are required to produce 1.0 × 108 kJ of energy?

 

Credits | Central iSchool | Sask Learning | Saskatchewan Evergreen Curriculum | Updated: 15-Jun-2006