Question Bank
1- How many grams of Carbon are in 16.55 g of glucose, C6H12O6.
2- Consider the following balanced equation:
6ClO2 + 3H2O  5HClO3 + HCl
What is the number of moles of HClO3 that are produced from
14.3 g of ClO2.
3- Consider the reaction:
Fe + 2HCl  FeCl2 + H2
What is the number of moles of H2 that will be formed if 0.40 mol
Fe and 0.75 mol of HCl are combined.
4- The number of grams of KNO3 which are needed to prepare 250
mL of 3.0x10-2 M KNO3 solution is………………….
(A) 0.7583
(B) 0.9650
(C) 2.3502
(D) 4.2156
5- What is the molarity of a solution that contains 49.0 g of H 2SO4 in
a 0.25 L of solution
6- How many glucose molecules C6H12O6 are in 5.23 g of it.
7- The volume of a gas is 750 mL at 75oC and 0.75 atm. At what
temperature (in oC) will the sample occupy 1.0 L under a
pressure of 1.0 atm. is ………….
(A) 217
(B) 117
(C) 246
(D) 346
8- How much water should be added to 12 M HCl to prepare 500 mL
of a 3.0 M HCl solution.
9- The oxidation number of P in Mg2P2O7 is……………….
(A) +2
(B) +6
(C) +5
(D) +10
10- Maliec acid contains 41.4% C, 3.45% H and 55.15% O by mass.
What is its simplest empirical formula
11-
How many moles of carbon are in 0.5 mol of CCl4 ?
12-
The empirical formula of an organic compound, that is
composed of 63.14% carbon, 5.31% hydrogen, and 31.55%
oxygen is:
(A) C4H4O
(B) C6H6O2
(C) C8H8O
(D) C8H8O3
13- Balance the following equation:
C2H6 + O2  CO2 + H2O
14- Assign oxidation number to each atom in the following:
a) OF2
b) H3PO4
c) PCl3
d) H2SO4
15- How many moles of oxygen are produced from the thermal
decomposition of 50.0g of Potassium chlorate according to the
following balanced equation.
2KClO3  2KCl + 3O2
16- The volume of sample of gas is 750 ml at 75 0C and 0.750 atm. At
what temperature will the sample occupy 1.00L under a pressure
of 1.00 atm?
17- Which of the following is a conjugate acid-base pair for the
reaction:
H3O+(aq) + NH3 (aq)  H2O(i) + NH +4 (aq)
a) H3O+, NH3
b) NH+4 , NH3 c) H3O+, OH-
d) H2O , NH3
18- How many molecules of (O2) are there in a sample of this gas
which occupies 11.2 l at STP?
19-The value of  H for the reaction:
2H2S (g) + 3O2 (g) → 2H2O (l) + 2SO2 (g)
a)  H =  E + RT
b)  H =  E + 3RT
c)  H =  E – R
d)  H =  E - 3RT
20- Given the following thermochemical reactions:
O3 + Cl  O2+ ClO
 H1= -126 KJ
Cl + O2  ClO + O
 H2= +268 KJ
Find the  H for the reaction :
O3 + O  2O2
21-  E of a gas for a process in which the gas absorbs 20 J of heat
and does 12 J of work by expanding is:
a) +8 J
b) –8J
c) +32 J
d) –32 J
22- How many grams of (SO2) are there in a 246 ml at STP?
23- How many atoms are there in 16.0 g S?
24- The empirical formula of the compound is C3H7 and the
molecular weight is 86.2 g. What is the molecular formula?
A)
C4H10
B)
C6H14
C)
C4H8
D)
C6H12
25- 5.0g of iron and 5.0g of Sulphur are heated together to form iron
sulphide which reactant is present in excess, and how much of
the product is formed ?
Fe(s) + S(s)  FeS(s)
26- Which of the following is the equation of state for a real gas?
A) PV = nRT
C)

n 2a 
 P  2 V  nb   nRT
V 

B)
P(V – nb) = nRT
D)

na 2 
 P  2 (V  nb)  nRT
V 

27- How many kilojoules of heat will raise the temperature of 3.0kg
of water from 22.00C to 25.00C if H2O = 4.184 J.g.-1 0C-1 ?
28- Which of the following compounds, the central atoms does not
obey the octet rule.
a) PCl3
b) H2O
c) IF7
d) CCl4
29- What is the density of NH3 (g) at 1000C and 1.51 atm ?
30- How many grams of Na2SO4 should be weighed to prepare 500 mL
of 0.1M solution ?
31-What is the molarity of a solution that contains 49.0 g of H 2SO4 in
a 0.25 L of solution?
a- One of the following should be a Lewis acid .
a) NH3
b) NF3
c) H2O
d) BF3
32- What pressure must be applied to 1.0L of a gas at 1.0
atmospheric
pressure to compress it to 0.40L ?
1- How many molecules of carbon are in 0.5 mol of CCl4 ?
2- The empirical formula of an organic compound, that is
composed of
63.14% carbon, 5.31% hydrogen, and
31.55% oxygen is:
(A) C4H4O
(B) C6H6O2
(C) C8H8O
(D) C8H8O3
3- Balance the following equation:
C2H6 + O2  CO2 + H2O
4- The oxidation number of carbon in acetone C3H6O is
(A) +1
(B) -1
(C) -4/3
(D) +3/2
5- How many moles of oxygen are produced from the thermal
decomposition of 50.0g of Potassium chlorate according to the
following balanced equation.
2KClO4  2KCl + 3O2
6- The volume of sample of gas is 750 ml at 755C and 0.750 atm. At
what temperature will the sample occupy 1.00L under a
pressure of 1.00 atm?
7- which of the following is a conjugate acid-base pair for the
reaction:
H3O+(aq) + NH3 (aq)  H2O(i) + NH +4 (aq)
a) H3O+, NH3
b) NH+4 , NH3 c) H3O+, OH-
d) H2O , NH3
8- How many molecules of (O2) are there in a sample of this gas
which occupies 11.2 l at STP?
9- The value of for the reaction:
2H2S (g) + 3O2 (g) → 2H2O (l) + 2SO2 (g)
a)  H =  E + RT
c)  H =  E – RT
b)  H =  E + 3RT
d)  H =  E - 3RT
10- Given the following thermochemical reactions:
O3 + Cl  O2+ ClO
 H1= -126 KJ
Cl + O2  ClO + O
 H2= +268 KJ
Find the  H for the reaction :
O3 + O  2O2
11-  E of a gas for a process in which the gas absorbs 20 J of heat
and does 12 J of work by expanding is:
b) –8J
a) +8 J
d) –32 J
c) +32 J
12- How many grams of (SO2) are there in a 246 ml at STP?
13- How much water should be added to 12 M HCl to prepare 500
mL of a 3.0 M HCl solution.
14- How many atoms are there in 16.0 g S?
15- The empirical formula of the compound is C3H7 and the
molecular weight is 86.2 g. What is the molecular formula?
A)
C4H10
B)
C6H14
C)
C4H8
D)
C6H12
16- If 0.06 mol of NaOH(aq) is mixed with 0.04 mol H3PO4(aq) and
allowed to react according to:
3 NaOH(aq) + H3PO4(aq)  Na3PO4(aq) + 3 H2O(l )
then the amount, in moles, of Na3PO4(aq) that should be
obtained is:
A)
0.06
B)
0.02
C)
0.04
D)
0.10
17- Which of the following is the equation of state for a real gas?
A)
PV = nRT
B)

n a
 P  2 V  nb   nRT
V 

P(V – nb) = nRT

na 2 
 P  2 (V  nb)  nRT
V 

2
C)
D)
18- How many kilojoules of heat will raise the temperature of 3.0kg
of water from 22.00C to 25.00C if H2O = 4.184 J.g.-1 0C-1 ?
19- which of the following compounds, the central atoms does not
obey the octet rule.
a) PCl3
b) H2O
c) IF7
d) CCl4
20- What is the density of HN3 (g) at 1000C and 1.51 atm ?
21- How many grams of Na2SO4 should be weighed out to prepare 500
mL of 0.1M solution ?
22-What is the molarity of a solution that contains 49.0 g of H 2SO4 in
a 0.25 L of solution?
23- How much water should be added to 12 M HCl to prepare 500
mL of a 3.0 M HCl solution. ?
24- The oxidation number of P in Mg2P2O7 is……………….
(A) +2
(B) +6
(C) +5
(D) +10
25- Maliec acid contains 41.4% C, 3.45% H and 55.15% O by mass.
What is its simplest empirical formula?
26- How many milliters of water must be added to 85.0 ml of 1.00M
H2SO4 to produce 0.650M H2SO4
27- one of the following would not serve as Lewis base .
a) NH3
b) NF3
c) H2O
d) BF3
28- What pressure must be applied to 1.0L of a gas at 1.0
atmospheric
pressure to compress it to 0.40L ?
29- What is the mass (in grams) of 6L of NH3 gas at STP?
30- How many molecules of (O2) are there in a sample of this gas
which occupies 11.2 l at STP?
31- complete the following:
 One mol of any gas at STP is = ------------------------ liter
  Hf for any element is = -------------------------------------- Ideal gas law equation is ------------------------------------------------ Dalton’s law equation is ------------------------------------------------ Hess’s law equation is ---------------------------------------------------31- The type of bond between two similar non-metallic atom is:
a) Apure ionic bond.
b) A pure covalent bond.
c) 50% ionic and 50% covalent.
d) No bond is formed.