Inorganic Chemistry Answers

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?

Given 0.2 M solution of NaCl in water with a specific gravity of 1.35.

• How many grams of NaCl are present in 800 mL of solution?
• What is the molality of the solution?

Find the molar concentration of a solution containing 8.56g of hydrogen chloride (HCL) in 500ml of solution

How many moles of Fe are needed to combine with 24 moles of Cl2 by this reaction? 

how much CuSo4x5H20 and how much H20 do you need to make 500g 10% CuSo4

b)  Answer the following stoichiometry questions by referring to the equation below:

2        KClO₃  ---->  2 KCl + 3 O₂

i.        If 1.50 mol of KClO₃ decomposes, what is the mass of O₂ that will be produced?

ii.       If 80.0 grams of O₂ was produced, how many moles of KClO₃ are decomposed?

iii.    Find the mass of KClO₃ needed if we need to produce 2.75 mol of KCl.