CHEM 1341 Exam 2 Review Game

Balancing Equations and Types of Reactions

100

Balance this Equation:

 _____ Al  +  _____ O2      →     _____Al2O3    

4, 3, 2

200

What type of reaction is this?

4Fe  +  3O2   ----->   2Fe2O3

Synthesis/Combination

300

What is the equation for Percent Composition?

𝑃𝑎𝑟𝑡/𝑊ℎ𝑜𝑙𝑒 ×100%

OR

 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑜𝑓 𝑖𝑛𝑡𝑒𝑟𝑒𝑠𝑡/𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑 ×100%

400

 What type of reaction is this?

3C  +  2Fe2O3   ----->   3CO2  +  2Fe

Single Replacement

500

Balance this equation

_____ AgNO3  +  _____ Ni      →     _____ Ni(NO3)2  +  _____Ag

2,1,1,2

Oxidation Numbers

100

What is the oxidation number for elements in their elemental state?

0

200

What is the oxidation number for hydrogen and oxygen?

Hydrogen is +1
Oxygen is -2

300

Tell me what OIL RIG is and tell me what oxidizing agents and reducing agents are.

-Oxidation is losing electrons = charge becomes more positive
-Reduction is gaining electrons = charge becomes more negative

-Oxidizing agent is the one that goes through reduction
-Reducing agent is the one that goes through oxidation  

400

What are the oxidation numbers for Sulfur and Oxygen?

                  S₂O₃^2- 

                 S _____ 

                 O ____

S: +2

O: -2

500

Determine which element is being oxidized and which element is being reduced in the following
reactions. Also balance the reaction.

___ NaClO₃(s)  ---->  ____ NaCl(s)  +  ____ O₂(g)

Coefficients: 2, 2, 3 

Oxidized: O

Reduced: Cl

Net and Total Ionic Equations

100

What is the difference between Net Ionic and Total Ionic Equations

Net Ionic Equations do not include spectator ions. while total ionic equations do.

200

What is a spectator ion?

An ion that does not participate in creating the precipitate

300

What is the precipitate in this reaction?

2KCl (aq) + Pb(NO₃)₂ (aq) -> 2KNO₃ (aq) + PbCl₂ (s)

PbCl₂(s)

400

What is the total ionic equation?

2KCl (aq) + Pb(NO₃)₂ (aq) -> 2KNO₃ (aq) + PbCl₂ (s)

2K⁺ (aq) + 2Cl^- (aq) + Pb₂⁺ (aq) + 2NO₃^– (aq) -> 2K⁺ (aq) + 2NO₃ ^– (aq) + PbCl₂ (s)

500

What is the Net Ionic Equation?

2KCl (aq) + Pb(NO₃)₂ (aq) -> 2KNO₃ (aq) + PbCl₂ (s)

2Cl^- (aq) + Pb₂⁺ (aq) -> PbCl₂ (s)

Solubility

100

Are nitrates always soluble?

Yes

200

Is ammonium always soluble?

Yes

300

Are hydroxides always soluble?

Hydroxides always insoluble EXCEPT with Group IA and NH4+, Ca, Sr, Ba

400

What is the weak base?

NH₃

500

Name all strong acids

1. HCl
2. HBr
3. HI
4. HNO3
5. HClO4
6. HClO3
7. H2SO4

Stoichiometry

100

 Calculate the number of grams of HCl that can react with 0.500 g of Al(OH)₃.

Al(OH)₃₍s)  +  HCl(aq)  →  AlCl₃(aq)  +  H₂O(l)

.701 g HCl

200

How many moles of O₂ are needed to burn 1.25 mol of C₈H₁₈?

2 C₈H₁₈(l)  + 25 O₂(g)  →  16 CO₂(g)  +  18 H₂O(g)

 

15.6 mol O₂

300

(Calculate the mass of calcium oxide that can be prepared from 4.20 g of solid calcium reacting with 2.80 g oxygen gas.  )

Determine limiting reactant by finding how many moles of O2 are needed to react completely with the
 moles of Ca that you have.  (Use mole ratio of reactants.) 

2 Ca(s)  +  O₂(g)  →  2 CaO(s)

Limiting: Ca

400

(Calculate the mass of calcium oxide that can be prepared from 4.20 g of solid calcium reacting with 2.80 g oxygen gas.)

 
Determine mass of CaO produced from the moles of limiting reactant that you have.

2 Ca(s)  +  O₂(g)  →  2 CaO(s)

5.88 g CaO

500

Calculate the mass of calcium oxide that can be prepared from 4.20 g of solid calcium reacting with 2.80 g oxygen gas. 

  Determine the mass of excess reactant that will react with the limiting reactant.  Subtract amount of
excess reactant that was used in the reaction from the amount that you have.

2 Ca(s)  +  O₂(g)  →  2 CaO(s)

1.12g O_{2 remains}