1. (a) Determine the amount of heat (in kJ) given off when 1.26 ×104 g of ammonia are produced from the following reaction:

N2 (g) + 3H2(g) → 2NH3(g); ?H°rxn = -92.6 kJ/mol

that the reaction takes place under standard conditions at 25°C.

(b) A 12.1 g piece of aluminum with a temperature of 81.7°C is added to a sample of water at 23.4°C in a constant-pressure calorimeter of negligible heat capacity. If the final temperature of water is 24.9°C, calculate the mass of the water in the calorimeter.

(c) Ethylene, C2H4, a compound with a carbon-carbon double bond, add hydrogen in a reaction called hydrogenation.

C2H4 (g) + H2(g) → C2H6(g)

Calculate the enthalpy change for this reaction, using the following combustion
data:

C2H4 (g) + 3O2(g) → 2CO2(g) + 2H2O(l); ?H = -1411 kJ
C2H6 (g) + 7/2O2(g) → 2CO2(g) + 3H2O(l); ?H = -1560 kJ
H2 (g) + 1/2O2(g) → H2O(l); ?H = -286 kJ

2. (a) Calculate the partial pressures of helium and neon after the stopcock of the following apparatus is open. Assume that the temperature remains constant at 16°C.

(b) The pressure of 6.0 L of an ideal gas in a flexible container is decreased to onethird of its original pressure, and its absolute temperature is decreased by onehalf. What is the final volume of the gas?

(c) Calculate the mass of water vaporized if 10.00 g of water is introduced into an evacuated flask of volume 2.500 L at 65°C. Assume that the volume of the remaining liquid water is negligible and the vapor pressure of water at 65°C is 187.5 mmHg.

3. (a) Sketch the phase diagram of argon, Ar, from the following information:

Normal melting point = -187°C
Normal boiling point = ?186°C
Triple point = ?189°C, 0.68 atm
Critical point = ?122°C, 48 atm

Label the triple point, critical point and each phase region in the diagram.

3(b) Which substance in each of the following pairs would you expect to have the higher boiling point? Explain why.

(i) Ne or Xe
(ii) CO2 or CS2
(iii) CH4 or Cl2
(iv) F2 or LiF
(v) NH3 or PH3

(c) Barium metal has a body-centered cubic lattice with all atoms at lattice points. Its density is 3.51 g/cm3 .From these data and the atomic weight, calculate the edge length of a unit cell.

4. (a) Calculate the valence electrons and draw complete Lewis structures, including lone pairs, for the following condensed structures:

(i) CH2CHCN
(ii) (HOCH2)2CO

(b) Write the resonance structure that would result from moving the electrons in the way indicated by the curved arrows:

(c) Draw the products of each Lewis acid-base reaction. Use curved arrows to show the movement of electrons in each reaction. Label the electrophile and nucleophile.

5. (a) By using compound A as a reference, label each compound as an isomer, a resonance structure, or neither. Explain your answer.

(b) Ketene, CH2=C=O, is an unusual organic molecule that has a single carbon atom doubly bonded to two different atoms. Determine the  hybridization of both C atoms and the O in ketene. Then, draw a diagram showing what orbitals are used to form each bond.

(c) There are two different substances with the formula C4H10. Draw both, and tell how they differ.