CHM 50Class Activity – Chapter 4Name

  1. Balance and indicate the type of reaction (double replacement, single replacement, combination, decomposition, precipitation, redox, combustion, gas evolution, acid-base neutralization) taking place. Multiple types can be applied.

a)____ NaBr(aq) + ____ H3PO4(aq) ____ Na3PO4(aq) + ____ HBr(aq)

Type of reaction: ______

b)____ Ca(OH)2(aq) + ____ Al2(SO4)3(aq)  ____ CaSO4(s) + ____ Al(OH)3(aq)

Type of reaction: ______

c)____ Mg(s) + ____ O2(g)  ____ MgO(s)

Type of reaction: ______

d)____ C2H4(g) + ____ O2(g)  ____ CO2(g) + ____ H2O(l)

Type of reaction: ______

e)____ PbSO4(s)  ____ PbSO3(s) + ____ O2(g)

Type of reaction: ______

f)____ NaN3(s)  ____Na(s) + ____ N2(g)

Type of reaction: ______

g)____ H2O(l)+ ____ SO3(g) ____ H2SO4(l)

Type of reaction: ______

  1. In the following redox reaction, identify which reactant is oxidized and which reactant is reduced
  1. 4 Al(s) + 3 O2(g)  2 Al2O3(s)Zn(s) + Fe2+(aq)  Zn2+(aq) + Fe(s)
  1. Zn(s) + Cl2(g)  ZnCl2(s)2Fe3+(aq) + Sn2+(aq)  2Fe2+(aq) + Sn4+(aq)
  1. Write an oxidation half and reduction half equation for the following redox reaction.
  1. Si(s) + 2F2(g)  SiF4(s)
  1. H2(g) + Cl2(g)  2HCl(g)

4.When MoO3 and Zn are heated together they react
3 Zn(s) + 2 MoO3(s) ------> Mo2O3(s) + 3 ZnO(s)
What mass of ZnO is formed when 20.0 grams of MoO3 is reacted with 10.0 grams of Zn?
5.Consider the reaction
I2O5(g) + 5 CO(g) ------> 5 CO2(g) + I2(g)
a)80.0 grams of iodine(V) oxide, I2O5, reacts with 28.0 grams of carbon monoxide, CO. Determine the mass of iodine I2, which could be produced?
b) If, in the above situation, only 0.160 moles, of iodine, I2 was produced.
i) what mass of iodine was produced?
ii) what percentage yield of iodine was produced.
6. Silver nitrate, AgNO3, reacts with ferric chloride, FeCl3, to give silver chloride, AgCl, and ferric nitrate, Fe(NO3)3. In a particular experiment, it was planned to mix a solution containing 25.0 g of AgNO3 with another solution containing 45.0 grams of FeCl3.
a)Write the chemical equation for the reaction.
b)Which reactant is the limiting reactant?
c)What is the maximum number of moles of AgCl that could be obtained from this mixture?
d)What is the maximum number of grams of AgCl that could be obtained?
e)How many grams of the reactant in excess will remain after the reaction is over?
  1. Calculate the molarity of each of the following solutions
  2. 22.6 g LiCl in a 2.8 L solution
  1. How many moles and grams of KCl are presented in each of the following
  2. 0.556 L of a 2.3 M KCl solution
  1. What volume (mL) is needed to obtain a solution of 0.750M Ca(NO3)2 in the present of 0.0450 moles of Ca(NO3)2?
  1. Calculate the final concentration when water is added to a 0.50L of a 12.0M KOH solution to make 4.5M of a diluted NaOH solution
  1. Calculate the number of mL of 2.00 M HNO3 solution required to react with 216 grams of Ag according to the equation.

3 Ag(s) + 4 HNO3(aq) ------> 3 AgNO3(aq) + NO(g) + 2 H2O(l)

  1. Calculate the number of grams of AgCl formed when 0.200 L of 0.200 M AgNO3 reacts with an excess of CaCl2. The equation is:

2 AgNO3(aq) + CaCl2(aq) ------> 2 AgCl(s) + Ca(NO3)2(aq)

  1. What volume of 0.415 M silver nitrate will be required to precipitate as silver bromide all the bromide

ion in 35.0 mL of 0.128 M calcium bromide?

2 AgNO3(aq) + CaBr2(aq)  Ca(NO3)2(aq) + 2 AgBr(s)

Dang1