The following results, in the table below, were obtained through a series of two

Question

The following results, in the table below, were obtained through a series of two experiments:

A) Write the total 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.

Experiment 1: Reactions w/ acids

Experiment 2: Replacement reactions

Cr2+ + 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.

Cr(s) Ag(s) HCl metal dissolves, bubbles, green solution no apparent reaction H2SO4 metal dissolves, bubbles, bluish purple solution no apparent reaction

Explanation / Answer

Exp1)

3HCl + Cr(s) --> Cr+3(aq) + 3/2H2(g) + 3Cl-(aq)

net ionic

3H+(aq) + Cr(s) --->  Cr+3(aq) + 3/2H2(g)

for..

3H2SO4 + 2Cr(s) ---> 3SO4-2(aq) + 3H2(g) + 2Cr+3(aq)

net ionic

6H+(aQ) + 2Cr(s) -->  3H2(g) + 2Cr+3(aq)

Exp2)

Cr+2 + Ag(s) --> no reaction

3Ag+(aq) + Cr(s) --> 3Ag(s) + Cr+3(aq)

this means that: Silver has a higher reduction potential

Silver is least active than chromium

Color change is due to the Appearance of Chrmoium ions in Cr+2 and Cr+3

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.