question archive Use both the metal and the halogen activity series to predict whether each of the following reactions will occur
Use both the metal and the halogen activity series to predict whether each of the following reactions will occur
Subject:ChemistryPrice:3.86 Bought8
Use both the metal and the halogen activity series to predict whether each of the following reactions will occur. Write the formulas for the products and balance the equation, if the reaction does take place.
a. AgNO3 + Zn →
b. Cl2 + NaI →
c. Fe + Al2 O3
Purchase A New Answer
Custom new solution created by our subject matter experts
GET A QUOTE
Answer Preview
a.) AgNO3(aq) + Zn(s)
When the solid metal (A) is above the metallic ion (B), the solid metal will displace the metallic ion.
A(s) + Bx+(aq) ----> Ay+(aq) + B(s)
Solid metal: Zn(s)
Dissolved metal: Ag+(aq)
Zinc is above silver, the reaction will proceed.
2AgNO3(aq) + Zn(s) ----> Zn(NO3)2(aq) + 2Ag(s)
b.) Cl2 + NaI
When the halogen gas (X2) is above the dissolved halide ion (Y-), the halogen gas will displace the dissolved halide ion.
X2(g) + Y-(aq) ----> X-(aq) + Y2(g)
Halogen gas = Cl2 (chlorine)
dissolved halogen ion = I- (iodide)
Since Chlorine is above iodine, chlorine gas will displace the dissolved iodide ion:
Cl2(g) + 2NaI(aq) -----> I2(s) + 2NaCl(aq)
c.) Fe(s) + Al2O3(aq)
Metal = Fe (iron)
dissolved metal ion = Al3+
Since Iron is below Aluminum, Iron will not be able to displace aluminum.
Fe(s) + Al2O3(aq) -----> NO REACTION
Please see the attached file for the complete solution
