Inorganic Chemistry Answers

1.   Transition metals are found in the centre section of the periodic table.

a)     Give two ways that transition metals are different to Group I metals?

b)     Give one way that transition metal compounds are different to Group I metal compounds.

calculate ΔH for the formation of one mole of dinitrogen pentoxide from its elements in their stable state at 25°C and 1 atm.

1. ____ Fe2O3 + ____ C → ____ Fe + ____ CO 
2. Balance the equation.
3. How many grams of carbon are needed to completely react with 125 g iron (III) oxide?

How many grams of h20 are produced from 0.25 moles of o2

How many grams of h20 are produced from 0.25 moles of o2

Sulfur (1400 kg) and pearl caustic soda (950 kg) are reacted to form sodium polysulphide (Na2Sx) to a total of 4000 L (balanced by H2O). What percentages (%) of total sulphur (S), sodium sulphide (Na2S), sodium thiosulphate (Na2S2O3) and sodium sulfur compounds are in solution?

 What is the acid disassociation expression for acetic acid (not the constant, but the equation)

Zn+AgCl

1. Assume that the Cu2+ + 2e- / Cu half reaction has an half-cell potential of 0.34 volts, using the data you obtained in Part IA on your observation sheet, calculate the half-cell potential for the voltaic cells containing the following electrodes: Cd, Pb, Zn  and Ag (show your work) (6 marks) 

1. From your response in 1 above, write out the half-cell equations as a reduction for each half cell (include the calculated redox potentials for each half cell equation) and place them in order starting with the strongest oxidizing agent including copper.(2 marks)

1. In Part I. C, you measured the voltaic cell potential between the Cu2+/Cu and the I2/I- half-cells. Report your observed cell potential and state which half-cell was the stronger oxidizing agent (1mark)

3b. From your response in 3 above, write the half-cell equation for each half-cell as a reduction and include the value of the half-cell potential for each equation. (1 mark)

1. In PART II you measured the cell potential between Cu/Cu2+ and Fe3+/Fe2+ using the value of the half-cell potential for Cu/Cu2+ of 0.34V, calculate the half-cell potential for the Fe3+/Fe2+half-cell. (2 marks)

5b.Name the electrode that was used in the Fe3+/Fe2+ half-cell and give two reasons why Fe(s) was not used. (0.5 mark)

1. Part IV. A. From your observation sheet report the colour changes in the DCM layer that were observed when FeCl3 was added to 0.2M KBr. (0.5 mark)

6b. Did a reaction take place? Write an equation for the REDOX REACTION. (0.5mark)

1. Part IV. A. From your observation sheet report the colour changes in the DCM  layer that were observed when FeCl3 was added to 0.1M KI. (0.5 marks)

7b. Did a reaction take place? Write an equation for the anode half-cell. (1mark)

1. GENERAL:

In this lab, you measured the cell potential between I2/I- and the Fe3+/Fe2+ half-cells, draw a diagram of the set up that you used. On the diagram, name and label the electrode where REDUCTION OCCURRED. Indicate the direction of electron flow in the circuit and clearly indicate how the ions (K+ and NO3-) flow in the salt bridge. (4 marks)

You have a 0.100mol piece of aluminum. How many atoms are present in the aluminum?