WORKSHEET#8 Homework, CHEM001   (Chapters 8 & 9)  

 Name: ____________________________   Date: ___________________  

1. Calculate the number of moles in 326 mg ZnCl 2 .       2. Balance and the following equations. Classify each reaction as synthesis, decomposition,  single-displacement, or double-displacement.   

a. ____PCl 5 + ____H 2 O ⎯→ ____POCl 3 + ____HCl      

  

b. ____Fe + ____O 2 ⎯→ ____Fe 2 O 3        

3. Use the activity series to predict which of the following reactions will occur. Complete  and balance the equations. If no reaction occurs, write “no reaction” as the product.   

a. ____Cu(s) + ____NiCl 2 (aq) ⎯→      

b. ____I 2 (s) + ____CaCl 2 (aq) ⎯→      

 

 

 

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ANSWER KEY

= (65.371+2135.45)=136.27 glmol

326mg x1

of ×

I mot

1000mg 136.27g= O' IIE39 Mol =2.39×10-3 mot

metals.

nonmetals,

H,

O

1 I 1 2

double - displacement

4 3 2

synthesis

- ~

nd Men

Ni > Cu

nomenw w

Clz> Iz

4. Balance the following equation. How many grams of H 2 O will be produced from the  neutralization of 26.35 g of NaOH in the presence of 12.50 g of H 2 SO 4 , and the reaction yield is  91.0%?   

NaOH + H 2 SO 4 ⎯→ H 2 O + Na 2 SO 4                

5. (9-12) Given the following equation, how many moles of water are needed to react with  101 g of Al 4 C 3 ?  

 

Al 4 C 3 + 12H 2 O ⎯→ 4Al(OH) 3 + 3CH 4  

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[ 211.01) -146.00 ) = 18.02 glmal H2O

5. X

↳ ( 22.997+(16.001+11.01)=40.00 glmol ↳ 211.01 ) -1 (32.017-1446.00)=98.03 glmol

2 2

LINA2 Na 2 Na

4 H#

4h

GO 60

26.35g NaOH xI Mol NaOH

= 0.6588 mot NaOH (need 0.255 male )

40.00g

12.50g HzS04 × I mot H 2504= 0.1275 mot Hzsoy ( have 0.1275 mal )

98.03g

0.1275 mot Hzsoy x

2 mot H2Ox 18.028 H2O = 4.595g H2O x 0.91 = 4.182

gH2O

1 mot Hzsoy I mot

4.

×

= 4126.98) -1342.01 ) = 143.95 glmol

101g Alycz x1 Mol At 403

×12 mot H2O

= 8.42 mot H2O

143.95g I mot Alyce

WORKSHEET#8, CHEM001   (Chapters 8 & 9)  

 Name: ____________________________   Date: ___________________ 1. Calculate the number of moles in 1.05 kg of NaHCO 3 .  

      

2. (8-4 & 8-22) Complete and balance each of the following equations. Classify each reaction as  synthesis, decomposition, single-displacement, or double-displacement. All reactions yield  products.   a. ____BaO 2 (s) + ____H 2 SO 4 (aq) ⎯→ ____BaSO 4 (s) + ____H 2 O 2 (aq)  

   

b. ____Ba(ClO 3 ) 2 ⎯ ⍙ → ____BaCl 2 + ____O 2    

c. ____CrCl 3 + ____AgNO 3 ⎯→ ____Cr(NO 3 ) 3 + ____AgCl   

 

3. (8-16) Use the activity series to predict which of the following reactions will occur. Complete  and balance the equations. If no reaction occurs, write “no reaction” as the product.   a. ____Mg(s) + ____Al(NO 3 ) 3 (aq) ⎯→  

   

b. ____FeCl2 + ____Zn ⎯→     

c. ____HNO3   + ____Au ⎯→      

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ANSWER HEY

↳ ( 22.99 ) -1 ( 1.01 ) -142.01 ) -1346.00 ) = 84.01 glmal

1.05kg x 1000g ×t mot Na # 003

= 12.50 mot NAHCOZ1kg 84.01g

I 1 I 1

double - displacement

I I 3 decomposition24 2cL

60 2X 60

1 3 I 3 double - displacement3 Cl

ICX 3cL

thy 3Ag 3 Ag

3 2 -2At + 3-Mg ( Nosh

I I 12inch -11Fe

2 2 2AuN0z t Hz

4. Balance the following equation. How many grams of Al 2 O 3 will be produced from the  oxidation of 18.15g of Al in the presence of 42.00g of Fe 2 O 3 , if the reaction yield is 80.0%?  

Al + Fe 2 O 3 ⎯→ Al 2 O 3 + Fe  

                

5. Given the following equation, how many moles of iron(III) oxide are needed to react with 32  g of carbon?  

Fe 2 O 3 + 3C ⎯ ⍙ → 2Fe + 3CO  

 

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g

2126.98) -1346.00 ) = 101.96 glmol

5. X

2 2↳ 2155.85 ) -13116.00 ) = 159.70 glmol

18.15g At x

t M "= 0.6727 mot At

26.98g

1 MOI= 0.2630 mot Fez Oz

,

REACTS WITH 0.526 mot OF At .42.00g Feds ×

159.70g

0.2630 mot Fezoz × 1 mot At 203× 101.96g At 203

= 26.82g A 12031 mot Feds I mot Ah 03 theoreticalyield

(26.82g) ( 0.80 ) = 21.45g of AKO ,

4

32g carbon x1 mot carbon

×

1 mot Feds= 0.89 mot Fezoz

12.01g carbon 3 mot carbon