Prepare your notebook for this experiment. Make tables that you can fill out whi
ID: 514837 • 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 experiment, 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 silver and chromium. Reactions with acids: 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
experiment No.1
2Cr(s) + 6Hcl (aq) ---------> 2CrCl3 (aq) + 3H2(g)
net ionic equation is
2Cr(s) + 6H+ (aq) ----------> 2Cr+3(aq) + 3H2(g)
experminent No.2
2Cr(s) + 3H2SO4 (aq) ---------> Cr2(SO4)3 (aq) + 3H2(g)
net ionic equation is
2Cr(s) + 6H+ (aq) ----------> 2Cr+3(aq) + 3H2(g)
b) When Cr metal becomes Cr+3 the color changes to bluish green int experiment 2
c) Based on these experminet we can say Cr is more reactive than Ag.
When Ag is dipped in Cr+3 solution where was n o reaction, but Cr in Ag+ solution , replaced Ag from solution to give Cr+3
Cr(s) + 3Ag+ (aq) ----------> Cr+3 (aq) + Ag(s)