Download CHE 145-381 – TEST #2 SPRING 2009 CHAPTERS 6, 7, 8 NAME

CHE 145-381 – TEST #2
SPRING 2009
CHAPTERS 6, 7, 8
NAME :________________________
DATE: ____________________________
You may use the Periodic Table. Please note that all quantities needed for the successful completion of
this test have been given. Feel free to ask questions for clarification.
1. Indicate to which of the following types of chemical reactions each of the statements listed
applies: synthesis, decomposition, single replacement, double replacement, or combustion.
a. two reactants are required ____________________________________________
b. only one reactant is present __________________________________________
c. two products are required ____________________________________________
d. only one product is present _______________________________________
2. Balance the following equations, and classify each of the reactions as (i) synthesis (ii) single
replacement (iii) double replacement (iv) decomposition of (v) combustion.
a.
C3H5O9N3 →
CO2 + N2 + O2 + H2O __________________
b.
C8H18 +
O2 →
CO2 +
H2O
___________________
c.
Al2O3 +
HNO3 →
Al(NO3)3 + H2O
___________________
d.
Na2CO3 +
H2O +
CO2 →
NaHCO3
____________________
e.
Co +
HCl
→
CoCl3 +
H2
____________________
3. Identify the products of, then write a balanced equation for each of the following:
a.
AlCl3 →
? +
?
(decomposition)
b.
Cu(NO3)2
+
c.
Al
+
Ni(NO3)2
d.
N2
+
H2
e.
C8H18
+
→
Na2CO3
→
→
O2
?
?
+
+
?
?
→
?
?
(double replacement)
(single replacement)
(synthesis)
+
?
(combustion)
4. You have one mole of each of the following substances:
cobalt (II) chloride
gold (III) chloride
ammonium phosphate
(a) write the chemical formula for each substance.
(b) which sample contains the greatest total number of atoms in one formula unit?
(c) which sample has the greatest mass?
5. Give the formula for each of the following:
1. acetic acid ____________
2. nitrous acid _______________
3. hypoiodous acid ________________
4. bromic acid _________________
5. bromous acid ________________
6. periodic acid ___________________
7. potassium hypobromite _________________
8. sodium perclorate __________________
9. titanium nitrite _________________
10. ammonium sulfite ________________
11. copper (I) phosphite _______________
12. lead (II) bromite ___________________
13. potassium hypochlorite _____________
14. gold (III) cyanide ________________
15. perbromic acid __________________
16. tin (IV) sulfide ________________
17. nitric acid ____________________
18. hydrochloric acid __________________
19. lead (IV) phosphate ___________________
20. iron (III) oxide _______________________
6. Name the following molecular compounds:
N2O5 __________________________________
NO ____________________________________
CBr4 ___________________________________
CO ________________________________________
N2O4 _______________________________________
SO3 ________________________________________
IF7 _____________________________________
NH3 _____________________________________
PH3 ______________________________________
HF (g) _______________________________________
H2S (g) _______________________________________
HBr (g) _______________________________________
7. How many grams are present in a sample of 5.743 x 1024 molecules of calcium nitrate?
8. Calculate the mass percent of nitrogen in 125g of CO(NH2)2.
8. Potassium thiosulfate, K2S2O3, reacts with chlorine, Cl2, and water in the following manner:
K2S2O3
+ 4Cl2
+ 5H2O →
2KHSO4
+ 8HCl
a. write the equation in words.
______________________________________________________________________
______________________________________________________________________
______________________________________________________________________
______________________________________________________________________
b. how many moles of each element are in 1 mole of K2S2O3? Write your answers in
the form of conversion factors.
___________________________________________________________________________
___________________________________________________________________________
___________________________________________________________________________
c. write all of the pertinent conversion factors based on this balanced equation for all
of the molar relationships between the reactants and products.
___________________________________________________________________
__________________________________________________________________
_
___________________________________________________________________
____________________________________________________________________
____________________________________________________________________
____________________________________________________________________
____________________________________________________________________
____________________________________________________________________
____________________________________________________________________
d. how many grams of Cl2 must react to produce 5.6 x 10 24 molecules of HCl?
e. how many moles of K2S2O3 must react to produce 25.0g of KHSO4?
f. how many grams of H2O must react to produce 20.00g of HCl?
g. how many molecules of HCl are produced at the same time that 2.000g of KHSO4 are
produced?