refers 1)
Precision to __________. A) how close a measured number B) how close a measured number C) how close a measured number D) how close a measured number E) how close a measured number
Answer: D
Page Ref: Sec. 1.4
is is is is is
to to to to to
the calculated value infinity the true value other measured numbers zero
2)
Accuracy refers to __________. A) how close a measured number B) how close a measured number C) how close a measured number D) how close a measured number E) how close a measured number
Answer: A
Page Ref: Sec. 1.4
is is is is is
to to to to to
the true value infinity zero other measured numbers the calculated value
3)
Which of the following has the same number of significant figures as the number 1.00310? A) 8.66 B) 5.119 C) 100 D) 199.791 E) 1 x 106
Answer: D
Page Ref: Sec. 1.4
4)
When the following equation is balanced, the coefficient of FeCl3 is __________. FeCl3 + Na2CO3 Fe2(CO3)3 + NaCl
A) 3 Answer: B
Page Ref: Sec. 3.1
B) 2
C) 4
D) 5
E) 1
5)
The compound responsible for the characteristic smell of garlic is allicin, C6H10OS2 . The mass of 1.00 mol of allicin is __________ g. A) 86 B) 19 C) 162 D) 34 E) 61
Answer: C
Page Ref: Sec. 3.4
1
6)
How many moles of carbon dioxide are there in 52.06 g of carbon dioxide? A) 8.648 x 1023 B) 3.134 x 1025 C) 1.183 D) 6.022 x 1023 E) 0.8452
Answer: C
Page Ref: Sec. 3.4
7)
Calculate the percentage by mass of nitrogen in PtCl2 (NH3)2. A) 4.95 B) 4.67 C) 9.34 D) 9.90
Answer: C
Page Ref: Sec. 2.4
E) 12.67
8)
Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2 (g) + 3H2 (g) 2NH3 (g) A 7.1-g sample of N2 requires __________ g of H2 for complete reaction. A) 0.51 B) 1.5 C) 1.2 D) 17.2 E) 0.76
Answer: B
Page Ref: Sec. 3.6
9)
How many grams of CH3OH must be added to water to prepare 150 mL of a solution that is 2.0 M CH3OH?
A) 4.3 B) 2.4 C) 4.3 D) 9.6 E) 9.6
x 102
x 103
Answer: D
Page Ref: Sec. 4.5
10)
How many moles of Co2+ are there in 0.200 L of a 0.400 M solution of CoI2? A) 2.00 B) 0.0800 C) 0.160 D) 0.500 E) 0.0400
Answer: B
Page Ref: Sec. 4.5
2
11)
The net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and aqueous nitric acid is __________. A) Al(OH)3 (s) + 3HNO3 (aq) 3H2O (l) + Al(NO3)3 (aq) (s) + 3NO3- (aq) 3OH- (aq) + Al(NO3)3 (s) C) Al(OH)3 (s) + 3HNO3 (aq) 3H2O (l) + Al3+ (aq) + NO3- (aq) D) Al(OH)3 (s) + 3NO3- (aq) 3OH- (aq) + Al(NO3)3 (aq)
B) Al(OH)3 E) Al(OH)3 Answer: E
Page Ref: Sec. 4.2
(s) + 3H+ (aq) 3H2O (l) + Al3+ (aq)
12)
What is molarity the of a NaOH solution if 28.2 mL of a 0.355 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution? A) 125 B) 0.400 C) 0.315 D) 0.801 E) 0.629
Answer: D
Page Ref: Sec. 4.6
13)
A 32.0 g sample of CH4O contains __________ molecules of CH4O. A) 1.00 B) 32.0 C) 6.02 x 1023 D) 1.88 x 1022 E) 5.32 x 10-23
Answer: C
Page Ref: Sec. 3.4
14)
What is the empirical formula of a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by mass? A) SO2Cl B) SOCl C) ClSO4 D) SOCl 2 E) S2OCl
Answer: D
Page Ref: Sec. 3.5
15)
How many milliliters of 0.132 M HClO4 solution are needed to neutralize 50.00 mL of 0.0789 M NaOH? A) 0.521 B) 29.9 C) 83.7 D) 0.0335 E) 0.0120
Answer: B
Page Ref: Sec. 4.6
3
16)
Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li (s) + N2 (g) 2Li3 N (s) In a particular experiment, 3.50-g samples of each reagent are reacted. The theoretical yield of lithium nitride is _________ g. A) 2.93 B) 17.6 C) 5.85 D) 3.52 E) 8.7
Answer: C
Page Ref: Sec. 3.7
17)
The density of silver is 10.5 g/cm3 . What volume (cm3 ) would be occupied by a piece of silver with a mass of 61.3 g? A) 644 B) 0.171 C) 10.5 D) 5.84 E) 0.00155
Answer: D
Page Ref: Sec. 1.4
18)
One mole of __________ contains the largest number of atoms. A) S8 B) C10H8 C) Na3PO4 D) Cl 2 E) Al2(SO4)3
Answer: B
Page Ref: Sec. 3.4
19)
How many atoms of nitrogen are in 10 g of NH4NO3? A) 1.5 x 1023 B) 3.0 x 1023 C) 1.8 D) 2 E) 3.5
Answer: A
Page Ref: Sec. 3.4
4
20)
Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: S (s) + 3F2 (g) SF6 (g)
In a particular experiment, the percent yield is 79.0%. This means that a 7.90-g sample of fluorine yields __________ g of SF6 in the presence of excess sulfur. A) 30.3 B) 0.110 C) 24.0 D) 10.1 E) 7.99
Answer: E
Page Ref: Sec. 3.7
21)
A strong electrolyte is one that __________ completely in solution. A) ionizes B) dissolves C) disappears D) reacts E) decomposes
Answer: A
Page Ref: Sec. 4.1
22)
Based on the equations below, which metal is the most active? Pb(NO3)2 (aq) + Ni (s) Ni(NO2)2 (aq) + Pb (s) Pb(NO3)2 (aq) + Ag (s) No reaction Cu(NO3)2 (aq) + Ag (s) No reaction
A) Cu Answer: B
Page Ref: Sec. 4.4
B) Ni
C) N
D) Ag
E) Pb
23)
__________ is an oxidation reaction. A) The reaction of sodium chloride with lead nitrate to form lead chloride and sodium nitrate B) Ice melting in a soft drink C) Neutralization of HCl by NaOH D) Table salt dissolving in water for cooking vegetables E) Rusting of iron
Answer: E
Page Ref: Sec. 4.6
5