Prepare your notebook for this experiment. Make tables that you can fill out whi
ID: 513034 • Letter: P
Question
Prepare your notebook for this experiment. Make tables that you can fill out while performing the procedure. You will be attempting a large number of reactions in this experiments and it is very important that you stay organized. You should make sure to leave plenty of room to record your observations. The following results, displayed in the table below, were obtained through a series of two experiments: a. Write the total and net ionic equations that describe all of the results noted from Experiment 1 and Experiment 2. b. Explain the color change observed in Experiment 2 (replacement reactions) c. Briefly discuss the relative activities of and chromium. Cr^2 + Ag metal: no apparent reaction, silver metal did not change, solution stayed green. Ag^+ Cr metal: silvery solid formed on piece of Cr metal. Solution went from colorless to bluish-green.Explanation / Answer
Answer:
a.
Total equation: Cr + 6HCl ------------> CrCl3 + 3H2
CrCl3 is the green colour compound formed this colour is due to presence of Cr 3+ ions.
Net Ionic: Cr + 3Cl- ---------> CrCl3
b. In this case Cr react with H2SO4 to form CrSO4
Cr + H2SO4 ------------> CrSO4 + H2
CrSO4 is the bluish colour compound formed this colour is due to presence of Cr 2+ ions
C.
The relative activity of chromium is more as compare to Ag because the position of Cr in electrochemical series is upper than Ag i.e. electrode potential of Cr is more than Ag