Student Assignment Samples

Sample Exams
(Chem. 10)

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Mid-term Exam I
Chem. 10

Summer 2000

How many significant figures are in 2.3450 * 10³?

2. Convert 123.5 ^oC to K

143.5 K
396.5 K
234.67 K
none of above

3. Convert 23.5 m to A^o.

1 A^o = 10^-10 cm

1m = 100 cm

2.35 * 10⁹ A^o
2.35 * 10¹³ A^o
2.35 * 10² A^o
none of above

4. A sample 2.43 g isopropyl alcohol is warmed by absorbing 3245.6 J of heat, How much does the temperature increase?

The specific heat of isopropyl alcohol is 2.51 J/ g. ^oC.

a. 532. ^o C

b. 144.3 ^o C

c. 223. ^o C

d. 678.9 ^o C

5. Which material is an element?

salt water
water
sulfur
sugar and water

6. Which material is a compound?

iron
oxygen
carbon dioxide
hydrogen

7. Which technique will you choose to separate a mixture of sulfur and water?

Sulfur is insoluble in water

filtration
cooling
mixing
none of above

8. The symbol for Neon is

9. The element of Ba is

nonmetal
metal
noble gas
none of above

10. Using the periodic table, the element in period 3 and IVA group is

11. How many electrons are in O^-2?

Atomic number of O = 8

12. What is the name of the element having the following masses and abundancy%?

Isotope mass amu Abundancy%

53.94 5.84

55.94 91.68

56.94 2.17

57.93 0.31

copper
iron
silicon
calcium

13. How neutrons are in ¹²₂₄Mg?

14. What is the formula for sulfur trioxide (more than one compound in the series)?

SO
SO₃
SO₂
SO₄

15. What is the formula for vanadium (II) sulfate?

V(SO₄)₂
V(SO₄)₃
VS
VSO₄

16. What is the name of the oxyacid derived from PO₃^-3?

Phosphoric acid
Phosphorous acid
phosphide
phosphorus

17. What is the name for Fe(NO₂)₃?

Iron nitrite
Iron (II) nitrite
Iron (III) nitrite
Iron (III) nitrate

18. What is the name for Mg(ClO₄)₂?

magnesium perchlorate
magnesium (II) perchlorate
magnesium chlorate
magnesium (II) chlorate

19. Which of the following reactions is balanced?

a. S + O_{2 =}SO₃

b. NaOH + Ba(OH)₂ = BaCl₂ + H₂O

c. CH₄ + O₂ = CO₂ + H₂O

d. CaCO₃ = CO₂ + CaO

20. Consider the following reaction:

AgNO₃ (aq) + HCl (aq) = AgCl (s) + HNO₃ (aq)

The reaction is

Single replacement
Combustion
Double repalcement
Decomposition

Key for Mid-term Exam I

1.a, 2.b, 3.b, 4.a, 5.c, 6.c, 7.a, 8.d, 9.b, 10.b, 11.b, 12.b, 13.b, 14.b, 15.d, 16.b, 17.c, 18.a, 19.d, 20.c

Mid-term Exam II

Chem. 10

Fall 1999

Each question has one point credit

How many protons and neutrons are in an atom of ²⁵₅₅Mn?

20 protons and 30 neutrons
15 protons and 30 neutrons
25 protons and 30 neutrons
none of above

2. How many electrons are in ³⁵₈₀Br atom?

30 electrons
35 electrons
80 electrons
45 electrons

3. What is the symbol for the isotope with 33 protons and 42 neutrons?

4. What is the element in group IIIA and period 4?

5. What is the atomic weight of potassium?

39.96 amu

39.10 amu

40.32 amu

40.56 amu

6. What type of element is N?

metal
noble gas
nonmetal
transition metal

7. Which of the following is the correct formula of fluorine gas found in the nature?

O
F
Cl₂
F₂

8. Which of the following is an oxyanion?

Cl^-
N₂
HBr
CrO₄^-2

9. Which of the following ions would form an ionic compound with ClO₃^-?

Br^-
O^-2
N^-3
None of above

10. A molecule of glucose is made of six carbon atoms, twelve hydrogen atoms and six oxygen atoms. What is the chemical formula of glucose?

C₆H₁₂O₆
CHO₂
C₃H₆O₃
CH₂O

11. What is the formula of the binary compound formed from the combination of I^- and Al⁺³?

AlI₂
AlI₃
AlI
AlI₄

12. What is the formula of the most likely ion to be formed from Li?

a. Li⁺²

b. Li⁺³

c. Li⁺

d. Li^-

13. What is the correct name of the compound having chemical formula of MnCl₂?

Manganese chloride
Manganese dichloride
Manganese (II) chloride
Manganese (III) chloride

14. What is the electrical charge (+charge) on Cu in the compound of Cu₂O?

–2
+2
–1
+1

15. What is the name for the compound whose formula is Ca(ClO)₂?

calcium chlorite
calcium dichlorite
calcium chlorate
calcium hypochlorite

16. What is the name for a compound whose formula is Fe(NO₂)₂

Iron (II) nitrate
Iron (II) nitrite
Iron nitrite
Iron (III) nitrite

17. What is the formula for the compound whose name is beryllium oxide?

BeO
BeO₂
Be₂O
BeO₃

18. What is the formula for the compound whose name is chromium (II) carbonate?

Cr(CO₃)₂
CrCO₃
Cr₂(CO₃)₃
Cr₂CO₃

19 .Name the oxyacid whose chemical formula is H₃PO₄

Phosphoric acid
Phosphorous acid
Phosphate acid
Phosphite acid

20.Write the formula of the oxyacid derived from sulfate (SO₄^-2) oxyanion.

HCl
HSO₃
H₂SO₃
H₂SO₄

21.Consider the following chemical reaction:

3CuO + 8HNO₃ = 3Cu(NO₃)₂ + 2NO + 4H₂O

What are the reactants?

a. 3Cu(NO₃)₂ + 2NO + 4H₂O

b. CuO + 2NO

c. 3CuO + 8HNO₃

d. 2NO + 4H₂O

22. Refer to the chemical equation:

CH₄ + O₂ = CO₂ + H₂O

In the correctly balanced equation, what are the coefficients for CH₄, O₂, CO₂ and H₂O, respectively?

1, 1, 1, and 2
1, 2, 1, and 2
1, 2, 1, and 1
2, 1, 2, and 1

23. Supply the missing coefficient and chemical formula in the following incomplete chemical equation.

--------+ O₂ = 2FeO

24.Which of the following reactions is balanced for the reaction between potassium oxide and water?

a. 2K + 2H₂O =2KOH + H₂

b. K₂O + 2H₂O₌2KOH

c. K₂O + H₂O = 2KOH

d. K₂O + 2H₂O = 2KOH + H₂

25.What type of chemical reaction is the following?

2NaOH + H₂SO_{4 =} Na₂SO₄ + 2H₂O

single replacement
combustion
decomposition
double replacement

26.What type of chemical reaction is the following?

2Na + Br₂ = 2NaBr

combination
decomposition
single replacement
double replacement

27. The chemical formula of propane is C₃H₈. What is the molecular weight of propane?

C= 12 amu, H = 1.0 amu

18 amu
34 amu
44 amu
none of above

28. What is the molar mass of Fe (OH)₃?

Fe = 56.0 g/mole, O=16.0 g/mole, H=1.00 g/mole

88 g/mole
333 amu
118 g/mole
107 g/mole

29. How many moles of O atoms are in 3.0 moles of C₁₂H₂₂O₁₁?

22 moles
24 moles
33 moles
44 moles

30. How many moles of NH₃ (ammonia) are contained in 15 g of ammonia?

N=14 g/mole, H=1.00 g/mole,

1 mole
3.2 moles
0.88 moles
1.4 moles

31. How many grams of FeCl₃ are contained in 0.64 moles of FeCl₃?

Fe = 56.0 g/mole, Cl = 35.5 g/mole

299 g
104 g
223 g
204 g

32.What is the mass percentage of oxygen in acetic acid (HC₂O₂H₃)?

C = 12.0 g/ mole, O = 16.0 g/mole, H = 1.00 g/mole

80%
33.5%
45.6%
53.3%

33.A compound has the following mass percentage composition: nitrogen=30.4, oxygen=69.6%. what is the empirical formula of this compound?

N=14.0 g/mole, O=16.0 g/mole

NO
N₂O
NO₂
N₂O₃

34.A compound has the empirical formula of C₅H₄O and the molecular weight of 240 amu. What is the molecular formula of this compound?

C=12.0 amu, H=1.00 amu, O=16.0 amu

C₅H₄O
C₅H₈O
C₁₅H₁₂O₃
C₁₀H₈O₂

Key for Mid-term exam II:

1.c, 2.b, 3.c, 4.a, 5.b, 6.c, 7.d, 8.d, 9.d, 10.a, 11.b, 12.c, 13.c, 14.d, 15.d, 16.b, 17.a, 18.b,

19.a, 20.d, 21.c, 22.b, 23.a, 24.c, 25.d, 26.a, 27.c, 28.d, 29.c, 30.c, 31.b, 32.d, 33. c,

34.c

Mid-term Exam III

Fall 1999

Chem.10.

How many moles of magnesium hydroxide (Mg(OH)₂) is required to neutralize 0.750 moles of HCl?

Mg(OH)₂ + 2HCl = MgCl₂ + 2H₂O

1.00
0.125
0.375
none of above

2. How many grams of Al will react with 3.45 moles of sulfuric acid?

2Al + 3H₂SO₄ = Al₂(SO₄)₃ + 3H₂

molar mass: Al =27.0 g/mole

62.1
33.2
78.9
100.1

3. Identify the limiting reactant if 3.2 moles NH₃ will react with 1.8 moles O₂.

4NH₃+ 5O₂ = 4NO + 6H₂O

NH₃
O₂
a, b
none of above

4. When 2.33 g Zn is burned in oxygen, how many grams of Zinc Oxide I s formed?

2Zn + O₂ = 2ZnO

Molar masses:

Zn = 65.0 g/mole, O = 16.0 g/mole

3.42 g
5.80 g
1.45 g
2.90 g

5. What is the electronic configuration of S^-2 ?

The atomic number of S is 16.

a.1s², 2s², 2p⁶, 3s², 3p⁴

b. 1s², 2s², 2p⁶, 3s², 3p⁶

c. 1s², 2s², 2p⁶, 3s², 3p⁵

none of above

6. How many p orbitals are in n = 3

7. What is the complete electronic configuration of ³⁸Sr?

[Ar] 4s²
[Ar] 4s¹
[Kr] 4s¹
[Kr] 5s²

8. Which is larger (larger atomic size), B or F?

F
Both F, B have the same atomic size
B
none of above

9. Which is smaller, As or As⁺³ ?

As⁺³
As
Both As and As⁺³have the same size
None of above

10. What is the valence electronic configuration of ¹⁷Cl?

3s², 3p⁵
1s², 2s², 2p⁶, 3s², 3p⁵
1s², 2s², 2p⁶, 3s², 3p⁴
3s², 3p⁴

11. What is the Lewis symbol for ¹⁵P?

12. What is the Lewis symbol for HOCl?

^{1H, ⁸O, ¹⁷Cl
a.
b.
c.
d.}

13. Which bond in each of the following pairs is more polar?

C – Cl and F – F

Electronegativity: F = 4.0, C =2.5, Cl = 3.0

F – F
Both C – Cl and F – F bnds
C – Cl
None of above

14. Determine the number of lone pair electrons in O = C = O (central atom) .

2
3
4
none of above

15.What is the type of bond in MgO?

covalent bond
ionic bond
both covalent and ionic bonds
none of above

16. What is the type of bond in SO₂?

covalent bond
ionic bond
both covalent and ionic bonds
none of above

17. What is the molecular shape of SH₂?

^{16S, ¹H

trigonal pyramidal
tetrahedral
trigonal planar
none of above

18. What is the molecular shape of PF₃?
^{15P, ⁹F

trigonal pyramidal
bent
tetrahedral
none of above

19. Which of the following is a polar molecule?
^{6C, ⁸O, ¹H, ¹⁷Cl, ⁹F

electronegativity: C = 2.5, O = 3.5, F = 4.0, Cl = 3.0, H = 2.1

CO₂

H₂

CCl₄

NF₃

20. What is the volume occupied by 3.20 g hydrogen at 22.0 C^o and 754 mmHg.
1 atm. = 760 mmHg, R = 0.08206 (L. atm. / K. mole)
molar mass of H = 1.008 g/mole

38.7 L.
38.7 ml.
100.2 L.
233.2 L.

21. Which gas will occupy the largest volume at STP?

1mole methane
2 moles fluorine
0.5 moles oxygen
1 mole hydrogen.

22. What is the partial pressure of N₂ if there is a mixture of N₂
and 0.44 moles CO₂ gasses in a 3.65 L. cylinder at 30 C^o and the
total pressure of 4.66 atm.
R = 0.08206 (L.atm. / K. moles)

2.33 atm.
1.66 atm.
3.22 atm.
None of above

23. A gas occupies 450 ml (cm³) at 2.34 atm. pressure. If the volume is
increases to 6.00 L (liter) at the same temperature and same amount of gas, what is the
new pressure?
1 L = 1000 ml.

0.175 atm.
1.22 atm.
2.33 atm.
none of above

24. If 1.00 g of oxygen occupies 0.700 L. at STP, what is the molar mass of this gas?

42.1 g/mole
63.9 g / mole
15.9 g/mole
none of above

25. Sulfur dioxide occupies 4.32 L. at 24 C^o and 746 mmHg. What is the new
temperature in C^o if the gas occupies 2.30 L. at 2.00 atm. The amount of sulfur
dioxide gas is constant.
1 atm. = 760 mmHg

56.2 C^o

49.2 C^o

122.0 C^o

33.2 C^o

key for Mid-term Exam III:
1.c, 2.a, 3.b, 4.d, 5.b, 6.b, 7.d.,
8.c, 9.a, 10.a, 11. Draw the Lewis symbol for P,
12. Draw the Lewis symbol for HClO, 13.c, 14.d, 15.
b, 16. a, 17. d, 18.a, 19.d, 20.a,
21. b, 22.b, 23.a, 24.d, 25. b

Mid-term Exam IV
Fall 1999
Chem. 10
1. How many milliters of 1.0 M KOH is needed to prepare 32.0 ml. of
0.11 M KOH?
a. 3.52 ml.
b. 4.33 ml.
c. 21.0 ml.
d. none of above.
2. Which of the following solid substance is a mettalic solid?
a. Xe
b. Cr
c. NaCl
d. none of above.
3. What is the correct expression for the equilibrium constant for the
following reaction?
H2(g) + I2(g) = 2HI(g)
a. K = [HI] / [H] [I]
b. K = [HI]2 / [H2] [I2]
c. K = [HI] / [H2] [I2]
d. none of above
4. Predict the direction of the following reaction if the concentration
of H2 is decreased.
2H2(g) + CO(g) = CH3OH(g)
a. the direction is shifted to the right side (product)
b. the reaction is shifted to the left side (reactants)
c. no change on the reaction
d. none of above

Key for mid-term exam IV:
1.a, 2.b, 3.b, 4.b

Final Exam
Chem. 10
Instructor: Lida L. Masoudipour, Ph.D.
Fall 1999
1.     Consider
the following process:
Water + sugar    =
   solution
The process is
a.      chemical
process
b.     physical
process
c.     combustion
reaction
d.     none of
above
2.     The room
temperature is in 25.0 C^o, the temperature on the Fahrenheit is
a.      77.0 ^oF
b.     88.4 ^oF
c.     111.0 ^oF
d.     none of
above
3.     In a
chemical process 123 kcal of heat has been produced. What is this heat in joules(J) = ?
1 kcal = 1000 cal,
            1cal = 4.18 J
a.      5.14
* 10⁵
b.     3.2 * 10³
c.     4.44 * 10⁶
d.     none of
above
4.
     How many electrons are in Cl^-?
¹⁷Cl
a.12
b.17
c.14
d.none of above
5.     What is the
element in the main group 3 (IIIA) and period 4?
a.      As
b.     Ge
c.     Al
d.     Ga
6.     How may
hydrogen atoms are in HCO₂H?
a.      1
b.     2
c.     3
d.     5
7.     What is the
formula of chromium (III) nitrite?
a. CrNO₃
b. Cr(NO₂)₃
c. Cr(NO₂)₂
d. Cr(NO₃)₃
8.     A molecule
consists of one carbon atom one hyrdogen atom, three oxygen atoms and one potassium atom.
What is the formula of this compound?
a. HCOK
b. HCO₂K
c. HCO₃K
d. none of above
9.     The formula
of monoatomic ion of Al is
a.      Al⁺³
b.     Al⁺²
c.     Al⁺
d.     None of
above
10. What are the correct coefficients for balancing the following
chemical reaction?
BaCO₃ + HCl =
BaCl₂ + CO₂ + H₂O
a.      1,1,1,1,1
b.     1,1,2,3,1
c.     1,2,1,1,1
d.     1,2,2,1,1
11.What type is the following chemical reaction?
CaCO₃ (s) = CaO
(s) + CO₂(g)
a.      combustion
b.     combination
c.     double
replacement
d.     none of
above
12.What are the products in the following reaction?
Ni (s) + 2HCl =
a.      NiCl
+ H
b.     NiCl₂
+ H₂
c.     NiClO + H
d.     None of
above.
13.A compound contains 38.7% K, 13.8% N and 47.5% O. What is the
empirical formula?
Molar masses:
       K = 39.0 g/mole,
    N = 14.0 g/mole,
    O = 16.0 g/mole
a.      KNO
b.     KNO₃
c.     KNO₂
d.     None of
above
14.What is the formula weight of NH₄H₂PO₄?
Atomic weights:
     N = 14.00 amu,
       H = 1.008 amu,
      O = 16.00 amu,
       P = 31.00 amu
a.      212.2
amu
b.     134 amu
c.     342 amu
d.     none of
above
15.How many moles of oxygen gas can you prepare from 1.22
moles of KClO₃?
2KClO_{3 =}2KCl
(s) + 3O₂ (g)
molar masses:
        K = 39.0 g/mole,    O = 16.0 g/mole,   Cl = 35.5 g/mole
a.      1.83
moles
b.     2.22 moles
c.     3.22 moles
d.     none of
above
16.How many grams of manganese (Mn) can be prepared from 50.0 g Al?
4Al(s) + 3MnO₂ = 2Al₂O₃
(s) + 3Mn(s)
molar masses:
        Al = 27.0 g/mole,   Mn = 55.0 g/mole,
           O = 16.0 g/mole
a.      76.4
g
b.     33.4 g
c.     112.0 g
d.     none of
above
17.What is the electronic configuration of K⁺?
a.      [Ne]
b.     [Ar]
c.     [Kr]
d.     none of
above
18.Which is smaller S or S^-2?
a.      S^-2
b.     S
c.     Both S and
S^-2
d.     none of
above
19. How many valence electrons are in C atom?
a.      1
b.     2
c.     4
d.     3
20.Which of the following is the correct electron – dot (Lewis
symbol) for PCl₃?
¹⁵P,
     ¹⁷Cl

a.

b.

c.

d.none of above
21. What is the volume in liter of 0.55 moles of hydrogen gas at 75
^o C and a pressure of 755 mmHg?
R = 0.0820 liter.atm/K.mole
1 atm. = 760 mmHg
a.      9.8
liter
b.     34.5 liter
c.     15.8 liter
d.     none of
above
22. which of the following gases can occupy the highest
volume at STP?
a.      1.0
mole hydrogen gas
b.     1.5 moles
fluorine gas
c.     2.0 moles
oxygen gas
d.     0.30 moles
of CH₄ (methane gas)
23. which molecule would have the strongest dispersion forces
between other identical molecules?
Atomic weighs:
      C = 12.0 amu,
       Cl = 35.5 amu,
       H = 1.00 amu,
       I = 126.9 amu,
       Br = 79.9 amu
⁶C,
     ¹H,
     ¹⁷Cl,
            ³⁵Br,
            ⁵³I
a.      CH₄
b.     CBr₄
c.     CCl₄
d.     CI₄
24. which of the following is an ionic solid?
a.      Ni
b.     KCl
c.     Xe
d.     None of
above
25. Which of the following best describes all the intermolecular
forces exhibited by a pure sample of CO₂?
Electronegativities: C = 2.5,       O = 3.5
⁶C,
     ⁸O
a.      Dipole
– dipole and hydrogen bonding
b.     Only
dispersion forces
c.     Dispersion
and dipole – dipole
d.     None of
above
26. How many milliliters of 5.0 M HCl
do you need to prepare 100.0 ml of 0.10 M HCl?
a.      34.0
ml.
b.     2.0 ml.
c.     10.0 ml.
d.     none of
above
27. How many moles are in 22.2 ml. of
2.05 M KOH?
1 liter = 1000 ml.
molar masses:
        K = 39.0 g/mole,    O = 16.0 g/mole    H = 1.00 g/mole
a.      1.22
moles
b.     0.0451
moles
c.     3.22 moles
d.     none of
above
28. what is the correct expression for
the equilibrium constant, K for the following
reaction?
2NO(g) + O₂(g) = 2NO₂(g)


a.      K =
[NO₂]² / [NO]² [O₂]
b.     K = [NO₂]
/ [NO]² [O₂]
c.     K = [NO]²
[O₂] / [NO₂]
d.     None of
above
29. Which
of the following sparingly soluble ionic substances (precipitates) is the most soluble?
a.      BaF₂
(K_sp = 1.7 * 10^-6)
b.     Ca₃(PO₄)₂
(K_sp = 2.0 * 10^-29)
c.     Zn₃(PO₄)₂
(K_sp = 9.0 * 10^-33)
d.     Sr F₂
(K_sp = 2.9 * 10^-9)
30. What is the conjugate acid of CN^-?
a.      HCN
b.     CN^-2
c.     CN^-3
d.     None of
above
31. Write the neutralization equation
for the reaction between sodium hydroxide and sulfuric acid.
a. NaOH + H₂SO₃ = H₂O + NaSO₃
b. 2NaOH + H₂SO_{3 =}H₂O + Na₂SO₃
c. 2NaOH + H₂SO_{4 =
   2}H₂O + Na₂SO₄
d.none of above
32. write the net ionic equation for
the reaction shown below:
BaCl₂(aq) + Na₂SO₄ (aq) = 2NaCl (aq) + BaSO₄ (s)
a. 2Cl^- (aq) + 2Na⁺ (aq) = 2NaCl(aq)
b. Ba⁺² (aq) + SO₄^-2 (aq) = BaSO₄ (s)
c. 2Cl^- (aq) + 2Na⁺ (aq) + Ba⁺²
(aq) + SO₄^-2 (aq) = 2NaCl
(aq) + BaSO₄ (s)
d.none of above
33. An
aqueous solution has the [H⁺] = 1.0 * 10^-5 M, the pH of solution is
a.      2.3
b.     4.3
c.     5.0
d.     none of
above
34. The pH of four solutions are given
below. What is the basic solution?
a.      pH =
2.0
b.     pH = 4.3
c.     pH = 7.0
d.     pH = 9.8
35. What is the oxidation number of V
in VO₂?
a.      –1
b.     +2
c.     +4
d.     +5
36. Identify the reducing agent in the following reaction:
I₂(aq) + 5Cl₂ (g) + 6H₂O = 10Cl^- (aq) + 2HIO₃ (aq) + 10H⁺
a.I₂
b. Cl₂
c. H₂O
d.non of above
37. Identify
the anode in the following reaction (use the activity series of metals)
3Ag⁺(aq) + Al(s) = Al⁺³
(aq) + 3Ag (s)
a.      Al
b.     Ag
c.     both Ag and
Al
d.     none of
above
38. Balance the following reaction
MnO₄^-+ Fe⁺²   = Fe⁺³ + Mn⁺²
The reaction occurs in acidic aqueous solution. The coefficient of
H⁺ in the balance equation is
a.      2
b.     8
c.     3
d.     non of
above

Key
for the final exam:
1.b,
2,a, 3.a, 4.d, 5.d, 6.b, 7.b, 8.c, 9.a,
10.c, 11.d, 12.b, 13.b, 14.d, 15.a, 16.a,
17.b,
18.b,
19.c, 20.Draw the Lewis symbole for PCl3, 21.c, 22.c, 23.d,
24.b, 25.b, 26.b, 27.b,
28.a,
29.a, 30.a, 31.c, 32.b, 33.c, 34.d, 35.c,
36.a, 37.a, 38.b

Final
Lab. Exam
Chem. 10
Instructor: Lida L. Masoudipour, Ph.D.
Fall 1999
Name:
1.     A titration
requires 22.38 ml. of 0.123 M NaOH. How many moles of NaOH are in this volume

2.     Balance the
following reactions:
a. BiCl₃(aq) + NaOH(aq) = NaCl (aq) + Bi(OH)₃(s)

b. Na₂CO₃(aq) + HNO₃ (aq) = NaNO₃ (aq) + CO₂ (g) + H₂O


3.     Write the
total ionic and net ionic equation for the following reaction:
AgNO₃ (aq) + HCl (aq) = AgCl
(s) + HNO₃ (aq)

4.     Write the
expression for the equilibrium constant for the following reaction:
NH₃(aq) + H₂O(l) = NH₄^- (aq) + OH^-
(aq)


Complete and balance the following reactions:
C(s) + O₂ (g) =
SO₂ (g) + H₂O
(l) =}}}

Sample Exams (Chem. 10)

Sample Exams
(Chem. 10)