Transcript Molar Relationships

Molar Relationships
The pH of a 0.1 molar
aqueous solution of
HCl would equal —
A
B
C
D
-1
1
11
13
If 3.50 g of H2S are used in the
above reaction, what will be the
theoretical yield of water in grams?
A
B
C
D
0.102 g
0.185 g
1.85 g
185 g
If 3.50 g of H2S are used in the
above reaction, what will be the
theoretical yield of water in grams?
3.5 gH2 S
1m olH2 S 2m olH2O 18gH2O
x
x
x
34.1gH2 S 2m olH2 S 1m olH2O
If 3.50 g of H2S are used in the
above reaction, what will be the
theoretical yield of water in grams?
A
B
C
D
0.102 g
0.185 g
1.85 g
185g
Which of the
following aqueous
solutions will
cause litmus paper
to turn red?
A
B
C
D
NaOH
NaCl
HCl
H2O
Which of the following
substances is a weak electrolyte?
A solution contains 225 g of
glucose, C6H12O6, dissolved in
enough water to make 0.825 L of
solution. What is the molarity of
the solution?
A
B
C
D
0.66 M
0.97 M
1.03 M
1.52 M
A solution contains 225 g of
glucose, C6H12O6, dissolved in
enough water to make 0.825 L of
solution. What is the molarity of
the solution?
m ol 225gC6 H12O6 1m olC6 H12O6
M

x
L
0.825L
180gC6 H12O6
A solution contains 225 g of
glucose, C6H12O6, dissolved in
enough water to make 0.825 L of
solution. What is the molarity of
the solution?
A
B
C
D
0.66 M
0.97 M
1.03 M
1.52 M
Carbon disulfide is prepared industrially
by reacting carbon with sulfur dioxide
according to the above equation. If 5.9
moles of carbon react, how many moles
of CS2 are produced?
A
C
0.077 moles
1.5 moles
B
D
1.2 moles
30 moles
Carbon disulfide is prepared industrially
by reacting carbon with sulfur dioxide
according to the above equation. If 5.9
moles of carbon react, how many moles
of CS2 are produced?
5.9m olC 1m olCS2
x

5m olC
Carbon disulfide is prepared industrially
by reacting carbon with sulfur dioxide
according to the above equation. If 5.9
moles of carbon react, how many moles
of CS2 are produced?
A
C
0.077 moles
1.5 moles
B
D
1.2 moles
30 moles
A solution which has a
concentration that exceeds its
predicted solubility at a certain
temperature and pressure would
be —
A
B
C
D
unsaturated
saturated
supersaturated
dilute
How many milliliters of 2.00 M
H2SO4 are needed to provide 0.250
mole of H2SO4?
A
B
C
D
125 mL
1.25 x 101 mL
8.00 x 103 mL
8.00 mL
How many milliliters of 2.00 M
H2SO4 are needed to provide 0.250
mole of H2SO4?
.250m olH2 SO4
1L
1000m L
x
x
2m olH2 SO4
1L
How many milliliters of 2.00 M
H2SO4 are needed to provide 0.250
mole of H2SO4?
A
B
C
D
125 mL
1.25 x 101 mL
8.00 x 103 mL
8.00 mL
What is the molarity of a solution
prepared by dissolving 27.2 g of
sodium chloride in enough water
to prepare 500.0 mL of solution?
A
B
C
D
0.186 M
0.465 M
0.930 M
1.860 M
What is the molarity of a solution
prepared by dissolving 27.2 g of
sodium chloride in enough water
to prepare 500.0 mL of solution?
m ol 27.2 gNaCl 1m olNaCl 1000m L
M

x
x

L
500.0m L 58.5 gNaCl
1l
What is the molarity of a solution
prepared by dissolving 27.2 g of
sodium chloride in enough water
to prepare 500.0 mL of solution?
A
B
C
D
0.186 M
0.465 M
0.930 M
1.860 M
When copper reacts with silver nitrate
according to the equation, the number
of grams of copper required to
produce 432 grams of silver is —
A
B
C
D
31.5 g
127 g
216 g
252 g
When copper reacts with silver nitrate
according to the equation, the number
of grams of copper required to
produce 432 grams of silver is —
432gAg 1m olAg 1m olCu 63.5 gCu
x
x
x

107.9 gAg 2m olAg 1m olCu
When copper reacts with silver nitrate
according to the equation, the number
of grams of copper required to
produce 432 grams of silver is —
A
B
C
D
31.5 g
127 g
216 g
252 g
What is the final concentration
if 50.0 mL of a 2.00 M solution
are diluted to 500.0 mL?
A
B
C
D
0.100 M
0.200 M
0.400 M
1.00 M
What is the final concentration
if 50.0 mL of a 2.00 M solution
are diluted to 500.0 mL?
M1V1  M 2V2
What is the final concentration
if 50.0 mL of a 2.00 M solution
are diluted to 500.0 mL?
M2
M1V1 2.00Mx50.0m L



V2
500.0m L
What is the final concentration
if 50.0 mL of a 2.00 M solution
are diluted to 500.0 mL?
A
B
C
D
0.100 M
0.200 M
0.400 M
1.00 M
The number of grams of oxygen
required for the complete
combustion of 4.00 grams of
methane (CH4) is —
A
B
C
D
4.00 g
8.00 g
16.0 g
32.0 g
The number of grams of oxygen
required for the complete
combustion of 4.00 grams of
methane (CH4) is —
4.00gCH4 1m olCH4 2m olO2 32gO2
x
x
x

16gCH4 1m olCH4 1m olO2
The number of grams of oxygen
required for the complete
combustion of 4.00 grams of
methane (CH4) is —
A
B
C
D
4.00 g
8.00 g
16.0 g
32.0 g
Zn + 2HCl → ZnCl2 + H2
If 0.600 gram of zinc is used, what
is the amount of zinc chloride that
is produced in the above reaction?
A
B
C
D
0.125 gram
1.25 grams
12.5 grams
0.018 gram
Zn + 2HCl → ZnCl2 + H2
If 0.600 gram of zinc is used, what
is the amount of zinc chloride that
is produced in the above reaction?
0.600gZn 1m olZn 1m olZnCl2 136.4 gZnCl2
x
x
x

65.4 gZn 1m olZn
1m olZnCl2
Zn + 2HCl → ZnCl2 + H2
If 0.600 gram of zinc is used, what
is the amount of zinc chloride that
is produced in the above reaction?
A
B
C
D
0.125 gram
1.25 grams
12.5 grams
0.018 gram
Four aqueous solutions and their
concentrations are shown in the above
illustration. Which of the solutions is most
likely to be the strongest conductor of
electricity?
A. I
B. II
C. III
D. IV
NaCl( s ) 
 Na
H 2O

( aq )
 Cl

( aq )
C6 H12O6 ( s ) 
 C6 H12O6 ( aq )
H 2O
I 2 x .5 or 1M
II 2 x 1.5 or 3M
III 1 x .5 or .5M
IV 1 x 1.5 or 1.5 M
Four aqueous solutions and their
concentrations are shown in the above
illustration. Which of the solutions is most
likely to be the strongest conductor of
electricity?
A. I
B. II
C. III
D. IV
In the reaction
2SO2 (g) + O2 (g)  2SO3 (g),
which change would cause the
greatest increase in the
concentration of SO3?
A
B
C
D
Decrease the concentration of SO2
Decrease the concentration of O2
Increase the concentration of SO2
Increase the concentration of O2
2H2(g) + 02(g)  2H2O(g)
How many liters of oxygen are required
to produce 2 liters of water at STP?
A
B
C
D
1
2
3
4
2H2(g) + 02(g)  2H2O(g)
How many liters of oxygen are required
to produce 2 liters of water at STP?
2 LH 2O
1m olH2O
1m olO2
22.4 LO2
x
x
x

22.4 LH 2O 2m olH2O 1m olO2
2H2(g) + 02(g)  2H2O(g)
How many liters of oxygen are required
to produce 2 liters of water at STP?
A
B
C
D
1
2
3
4
The molar volume of an ideal
gas in liters at STP is —
A
B
C
D
6.02 x 1023 L
11.2 L
22.4 L
0.0821 L
What is the density of carbon
dioxide at STP?
A
B
C
D
1.96 g/L
22.0 g/
46.0 g/L
5.09 x 10-1 g/L
m
D
V
What is the density of carbon
dioxide at STP?
Carbon Dioxide is CO2
Mass CO2 = 1(12.0) + 2(16.0) = 44.0g
Volume at STP is 22.4L
m 44 .0 g
D 

V 22 .4 L
What is the density of carbon
dioxide at STP?
A
B
C
D
1.96 g/L
22.0 g/
46.0 g/L
5.09 x 10-1 g/L
Which of these is about 2 moles?
A
B
C
D
2.0 liters (dm3) of H2
4.0 grams of H2
2.0 x 1023 molecules of H2
4.0 kilograms of H2
Which of these is about 2 moles?
2 mol of a gas (STP) = 2(22.4 L)
2 mol = 2(6.02 x 1023)
2 mol = 2(2.0g)
Which of these is about 2 moles?
A
B
C
D
2.0 liters (dm3) of H2
4.0 grams of H2
2.0 x 1023 molecules of H2
4.0 kilograms of H2
When magnesium metal (Mg) is
burned, it forms MgO. How many
moles of oxygen gas (O2) are
needed to burn 10 moles of Mg?
A
B
C
D
2
5
10
20
When magnesium metal (Mg) is
burned, it forms MgO. How many
moles of oxygen gas (O2) are
needed to burn 10 moles of Mg?
2Mg  O2  2MgO
10m olMg 1m olO2
x

2m olMg
When magnesium metal (Mg) is
burned, it forms MgO. How many
moles of oxygen gas (O2) are
needed to burn 10 moles of Mg?
A
B
C
D
2
5
10
20
Nitrogen gas is a diatomic
molecule. What is the mass of
one mole of nitrogen gas?
A
B
C
D
7g
14 g
28 g
6 x 1023 g
Nitrogen gas is a diatomic
molecule. What is the mass of
one mole of nitrogen gas?
Molar mass from Periodic Table
N2
2(14.0 g) =
Nitrogen gas is a diatomic
molecule. What is the mass of
one mole of nitrogen gas?
A
B
C
D
7g
14 g
28 g
6 x 1023 g
Which volume will be occupied
23
by a gas containing 6.02 x 10
atoms at STP?
A
B
C
D
1.0 L
11.2 L
22.4 L
44.8 L
Which volume will be occupied
23
by a gas containing 6.02 x 10
atoms at STP?
6.02 x 1023 = 1 mol
1 mol gas = 22.4 L
Which volume will be occupied
23
by a gas containing 6.02 x 10
atoms at STP?
A
B
C
D
1.0 L
11.2 L
22.4 L
44.8 L
Ulcers are often caused by an excess
of stomach acid. Milk of magnesia is
often used to soothe the irritation.
Milk of magnesia is probably —
A
B
C
D
an acid
a base
an indicator
a colloid
The hydrogen ion concentration is
1 x 10-7. What is the pH of this
solution?
A
B
C
D
1
7
10
14
How many grams of sodium chloride are
required to prepare 500.0 mL of a 0.100
M solution?
A. 1.46 g
B. 2.93 g
C. 29.3 g
D. 58.5 g
How many grams of sodium chloride are
required to prepare 500.0 mL of a 0.100
M solution?
1L
0.100 molNaCl 58.5 gNaCl
500 .0mLx
x
x

1000 ml
1l
1mol
A. 1.46 g
B. 2.93 g
C. 29.3 g
D. 58.5 g
2KOH + H2SO4 → 2H2O + K2SO4
What mass of potassium hydroxide is
required to react completely with 2.70 g of
sulfuric acid to produce potassium sulfate
and water?
A. 4.73 g
B. 3.09 g
C. 2.36 g
D. 1.54 g
2KOH + H2SO4 → 2H2O + K2SO4
What mass of potassium hydroxide is
required to react completely with 2.70 g of
sulfuric acid to produce potassium sulfate
and water?
1m olH2 SO4 2m olKOH 56.1gKOH
2.70gH2 SO4 x
x
x

98.1gH2 SO4 1m olH2 SO4 1m olKOH
A. 4.73 g
B. 3.09 g
C. 2.36 g
D. 1.54 g
W+X→Y+Z
How many grams of product Z will be
formed if 12.0 g of W react with 10.0 g of X
to form 8.0 g of product Y in the reaction
shown?
A. 8.0 g
B. 10.0 g
C. 12.0 g
D. 14.0 g
Remember Conservation of Mass
12 + 10 = Z + 8
22-8 = z
N2 + 3H2 → 2NH3
If 6 liters of hydrogen gas are used,
how many liters of nitrogen gas will be
needed for the above reaction at STP?
A. 2 liters 6LH x 1m olH2 x 1m olN2 x 22.4LN 2 
2
22.4 LH 2 3m olH2 1m olN2
B. 3 liters
C. 4 liters
D. 12 liters
The gas with the largest volume at
STP is —
A. 10.0 g He
B. 10.0 g Ne
C. 10.0 g Ar
D. 10.0 g Kr
The gas with the largest volume at
STP is —
1m olHe
10.0 gHex
 2.50m olHe
4 gHe
1m olNe
10.0 gNex
 0.500m olNe
20.2 gNe
1m olAr
10.0 gArx
 0.251m olAr
39.9 gAre
1m olKr
10.0 gKrx
 0.122m olKr
83.8 gKre
The gas with the largest volume at
STP is —
A. 10.0 g He
B. 10.0 g Ne
C. 10.0 g Ar
D. 10.0 g Kr
A has the greatest amount
of moles therefore it has
the largest volume
Which pair of solutions would be
acidic if mixed in equal quantities?
Solution A
pH
2
A. A and B
B. B and C
C. B and D
D. C and D
B
6
2 + 6 = 8/2 = 4
6 + 9 = 15/2 = 7.5
6 + 12 = 18/2 = 9
9 + 12 =21/2 =10.5
C
9
D
12
What is represented by the pH of a solution?
A. Partial pressure of hydrogen ions in the
solution
B. Electronegativity of dissociated hydrogen
ions in the solution
C. Concentration of hydrogen ions in the
solution
D. Temperature of hydrogen ions in the
solution
A container holds 20.0 grams of neon gas.
Under the same conditions, how many
grams of xenon would the container hold?
A. 108 g
B. 131 g
C. 262 g
D. 370 g
20.0 g Ne is about 1 mole therefore they
container would also hold 1 mole of Xeon
under the same conditions therefore the mass of
Xeon in the container would be about ……
How many grams of nitrogen are
present in 2 moles of HNO3?
A. 1
B. 2
C. 14
D. 28
If you have 2 moles of HNO3 that means
you have 2 moles of N.
2(14) =
Which is the base in the reaction?
A. H2O
B. KOH
C. K+
D. H2SO4
Produces OH- ions, or accepts a hydrogen
How many moles of copper are
equivalent to 3.44 x 1023 atoms of
copper?
A. 0.571 moles
B. 1.75 moles
C. 5.41 x 1021 moles
D. 5.71 x 1022 moles
6.02 x 1023 atoms of copper
= 1 mole of copper
Which condition will cause a shift in
the equilibrium of the above reaction?
A. Double the concentration of reactants and
products
B. Increase the reaction temperature
C. Reduce the concentration of products and
reactants by 10%
D. Keep the reaction temperature constant
What is the molar mass of Al(NO3)3?
A. 57 g/mol
B. 103 g/mol
C. 165 g/mol
D. 213 g/mol
1(27) + 3(14) + 9(16) =
What is the mass in grams of one
mole of sulfur dioxide (SO2)?
A. 48.1 g
B. 64.1 g
C. 80.1 g
D. 96.1 g
1(32.1) + 2(16) =
Formaldehyde (H2CO) reacts with
oxygen to form CO2 and H2O. How
many moles of CO2 will be produced
from reacting 2 moles of H2CO with
oxygen?
H2CO + O2  CO2 + H2O
A. 1
B. 2
C. 4
D. 8
It is a 1:1 ratio therefore ….
In the combustion of ethane, how
many moles of CO2 can be produced
from 1.00 mole of C2H6?
2C2H6 + 7O2  4CO2 + 6H2O
A. 0.500 mole
B. 1.00 mole
C. 2.00 moles
D. 4.00 moles
4m olCO2
1.00m olC2 H 6 x

2m olC2 H 6
The End