1. Suppose we titrate 20.00 mL sodium hydroxide with 0.972 M hydrochloric acid. If it takes 18.56 mL of acid of to neutralize the base, what is the concentration of the sodium hydroxide solution?
2. Suppose we oxidize 27.00 mL of iron (II) sulfate with potassium permanagnate solution in acid. If the iron sulfate solution is 0.0912 M, and the potassium permanagante is 0.21 M, how much permanganate will be needed? What indicator is used to detect the endpoint?
3. Zinc reacts with steam to generate hydrogen gas. Copper does not react with hydrochloric acid. Write a balanced equation to show the use of one as a reducing agent to reduce the other, in agreement with the electrochemical series.
4. Sodium reacts with cold water to generate hydrogen gas. Aluminum only generates hydrogen gas when reacting with steam. Write a balanced equation to show the use of one as a reducing agent to reduce the other, in agreement with the electrochemical series.
5. 44.01 g of CO2 occupies 37.03 cm3 at a pressure of 200 Torr. What is the temperature in degress Celsius?
6. A solution of KCl is reacted with silver nitrate to precipitate the chloride, and the white solid produced is dried in an oven overnight in a crucible. If 0.3562 g of solid remain, how much KCl was in the initial KCl solution?
7. Find the mean square speed of oxygen molecules at 400 ºC.
8. Write the van der Waals equation, and show which term is the attractive term, and which is the correction factor for non-zero molecular volume.
9. 2.50 × 102 ml of 1.00 M HCl reacts with 4.00 x 102 of 0.5 M NaOH in a constant pressure calorimeter with negligible (virtually zero) heat capacity. The enthalpy of reaction for the process H+1(aq) + OH-1 &rarr H2O(l) is -56.2 kJ/mol. What is the final temperature of the solution, if the initial temperature was 22.4 ºC?
10. 41.3 g of unknown metal at 76 ºC is placed in a constant pressure calorimeter that contains 100.0 g of water at 23.1 ºC. The calorimeter is at the same temperature as the water. The heat capacity of the calorimeter itself is 15.77 J/ºC, and the heat cpacity of the water is 4.186 J/ºC. The final temperature of the system is 29.4 ºC. What is the heat capacity of the metal?
11. Find the enthalphy of formation for CO2, using the fact that C (graphite) + O2 &rarr CO2, and the enthalpy of the reaction is -393.5 kJ/mol.
12. Find the energy of a photon of wavelength 567 nm, and its momentum.
13. What is the de Broglie wavelength of a American football weighing 400 g with velocity 40 m/s ?
14. What is the de Broglie wavelength of an electron (mass = 9.109 × 10-28 g), with velocity 1.0 × 108 m/s?
15. What are ALL the quantum numbers for the following orbitals: (a) 3p, (b) 4f, (c) 2d, (d) 2p.
16. Draw an energy diagram for the hydrogen atom, including all orbitals up to the n=6 level. Then draw an energy diagram for a NON-hydrogen atom, again up to the n=6 level.
17. Write the equation for the (first) ionization of F. Which element has the largest first ionization energy, and why?
18. Find the energy of a photon emitted from a hydrogen atom when an electron falls from the n=5 level to the n=1 level.
19. Give examples of acidic, amphoteric, and basic oxides.
20. Write the equations to define ionization energy and electron affinity.
© 2005 by Lawrence T. Sein. All rights reserved.
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