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41 Cards in this Set
- Front
- Back
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A nitrogen oxide is 63.65% by mass nitrogen. The molecular formula could be ________.
A) N2O4 B) N2O C) NO2 D) NO E) either NO2 or N2O4 |
B
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A sulfur oxide is 50.0% by mass sulfur. This molecular formula could be ________.
A) S2O B) SO2 C) S2O4 D) SO E) either SO2 or S2O4 |
E
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Which hydrocarbon pair below have identical mass percentage of C?
A) C2H4 and C3H4 B) C2H4 and C3H6 C) C3H4 and C3H6 D) C2H4 and C4H2 E) None of the above |
B
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When the following equation is balanced, the coefficients are ________.
NH3 (g) + O2 (g) → NO2 (g) + H2O (g) A) 4, 7, 4, 6 B) 2, 3, 2, 3 C) 1, 3, 1, 2 D) 1, 1, 1, 1 E) 4, 3, 4, 3 |
A
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When the following equation is balanced, the coefficients are ________.
Al(NO3) 3 + Na2S → Al2S3 + NaNO3 A) 2, 3, 1, 6 B) 1, 1, 1, 1 C) 2, 1, 3, 2 D) 2, 3, 2, 3 E) 4, 6, 3, 2 |
A
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When the following equation is balanced, the coefficient of H2 is ________.
K (s) + H2O (l) → KOH (aq) + H2 (g) A) 5 B) 1 C) 3 D) 4 E) 2 |
B
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When the following equation is balanced, the coefficient of Al is ________.
Al (s) + H2O (l) → Al(OH)3 (s) + H2 (g) A) 1 B) 2 C) 3 D) 4 E) 5 |
B
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When the following equation is balanced, the coefficient of H2S is ________.
FeCl3 (aq) + H2S (g) → Fe2S3 (s) + HCl (aq) A) 2 B) 3 C) 5 D) 4 E) 1 |
B
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When the following equation is balanced, the coefficient of C3H8O3 is ________.
C3H8O3 (g) + O2 (g) → CO2 (g) + H2O (g) A) 7 B) 5 C) 2 D) 3 E) 1 |
C
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When the following equation is balanced, the coefficient of H2 is ________.
CO (g) + H2 (g) → H2O (g) + CH4 (g) A) 0 B) 2 C) 4 D) 3 E) 1 |
D
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Write the balanced equation for the reaction that occurs when methanol, CH3OH (l) is burned in
air. What is the coefficient of methanol in the balanced equation? A) 2 B) 3/2 C) 1 D) 4 E) 3 |
A
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What is the coefficient of O2 when the following equation is completed and balanced?
C4H8O2 + O2 → ________ A) 1 B) 2 C) 3 D) 5 E) 6 |
D
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The balanced equation for the decomposition of sodium azide is ________.
A) 2NaN3 (s) → Na2 (s) + 3N2 (g) B) NaN3 (s) → Na (s) + N2 (g) C) 2NaN3 (s) → 2Na (s) + 3N2 (g) D) 2NaN3 (s) → 2Na (s) + 2N2 (g) E) NaN3 (s) → Na (s) + N2 (g) + N (g) |
C
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There are ________ hydrogen atoms in 25 molecules of C4H4S2.
A) 100 B) 25 C) 1.5 × 1025 D) 3.8 × 1024 E) 6.0 × 1025 14 |
A
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A sample of C3H8O that contains 200 molecules contains ________ carbon atoms.
A) 200 B) 3.61 × 1026 C) 600 D) 1.20 × 1026 E) 4.01 × 1025 |
C
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) How many grams of hydrogen are in 46 g of CH4O?
A) 184 B) 1.5 C) 5.8 D) 0.36 E) 2.8 |
C
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How many grams of oxygen are in 65 g of C2H2O2?
A) 130 B) 29 C) 18 D) 9.0 E) 36 |
E
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How many moles of carbon dioxide are there in 52.06 g of carbon dioxide?
A) 8.648 × 1023 B) 1.183 C) 0.8452 D) 6.022 × 1023 E) 3.134 × 1023 |
B
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A 2.25 g sample of magnesium nitrate, Mg(NO3)
2 , contains ________ mol of this compound. A) 0.0261 B) 65.8 C) 38.4 D) 0.0152 E) 148.3 |
D
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What is the empirical formula of a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by
mass? A) SOCl B) SOCl2 C) SO2Cl D) ClSO4 E) S2OCl |
B
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A compound contains 40.0% C, 6.71% H, and 53.29% O by mass. The molecular weight of the
compound is 60.05 u. The molecular formula of this compound is ________. A) C2H3O4 B) CHO2 C) C2H4O2 D) CH2O E) C2H2O4 |
C
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A compound that is composed of only carbon and hydrogen contains 85.7% C and 14.3% H by
mass. What is the empirical formula of the compound? A) C4H8 B) C2H4 C) CH2 D) CH4 E) C86H14 |
C
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A compound is composed of only C, H, and O. The combustion of a 0.519 g sample of the
compound yields 1.24 g of CO2 and 0.255 g of H2O What is the empirical formula of the compound? A) C3H3O B) C2H6O5 C) CH3O D) C2H6O2 E) C6H6O |
A
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Magnesium and nitrogen react in a combination reaction to produce magnesium nitride:
3Mg + N2 → Mg3N2 In a particular experiment, a 9.27 g sample of N2 reacts completely. The mass of Mg consumed is ________ g. A) 16.1 B) 24.1 C) 13.9 D) 8.04 E) 0.92 |
B
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The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O:
4NH3 (g) + 7O2 (g) → 4NO2 (g) + 6H2O (g) The combustion of 43.9 g of ammonia produces ________ g of NO2. A) 0.954 B) 2.58 C) 119 D) 43.9 E) 178 |
C
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Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2):
CaC2 (s) + 2H2O (g) → Ca(OH)2 (s) + C2H2 (g) Production of 13g of C2H2 requires consumption of ________ g of H2O. A) 4.5 B) 18 C) 4.8 × 10-2 D) 4.8 × 102 E) 9.0 |
B
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The mass of hydrogen produced by the reaction of 4.73 g of magnesium with 1.83 g of water is
________ g. Mg (s) + 2H2O (l) → Mg(OH)2 (s) + H2 (g) A) 0.0485 B) 0.102 C) 0.204 D) 0.0162 E) 0.219 |
B
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A 3.82 g sample of magnesium nitride is reacted with 7.73 g of water.
Mg3N2 + 3H2O → 2NH3 + 3MgO The yield of MgO is 3.60 g. The percentage yield of the reaction is ________% . A) 94.5 B) 49.4 C) 99.9 D) 78.8 E) 46.6 |
D
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Solid aluminium and gaseous oxygen react in a combination reaction to produce aluminium oxide:
4Al (s) + 3O2 (g) → 2Al2O3 (s) The maximum amount of Al2O3 that can be produced from 2.5 g of Al and 2.5 g of O2 is ________ g. A) 9.4 B) 7.4 C) 4.7 D) 5.0 E) 5.3 |
C
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Solid aluminium and gaseous oxygen react in a combination reaction to produce aluminium oxide:
4Al (s) + 3O2 (g) → 2Al2O3 (s) In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of O2 produced 3.5 g of Al2O3. The % yield of the reaction is ________. A) 47 B) 26 C) 37 D) 74 E) 66 |
D
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Which of the following are combination reactions?
1) CH4 (g) + O2 (g) → CO2 (g) + H2O (l) 2) CaO (s) + CO2 (g) → CaCO3 (s) 3) Mg (s) + O2 (g) → MgO (s) 4) PbCO3 (s) → PbO (s) + CO2 (g) A) 2 and 3 B) 4 C) 2, 3, and 4 D) 1, 2, 3, and 4 E) 1, 2, and 3 |
A
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Which of the following are combustion reactions?
1) CH4 (g) + O2 (g) → CO2 (g) + H2O (l) 2) CaO (s) + CO2 (g) → CaCO3 (s) 3) PbCO3 (s) → PbO (s) + CO2 (g) 4) CH3OH (l) + O2 (g) → CO2 (g) + H2O (l) A) 1 and 4 B) 1, 2, 3, and 4 C) 3 and 4 D) 1, 3, and 4 E) 2, 3, and 4 |
A
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Which of the following are decomposition reactions?
1) CH4 (g) + O2 (g) → CO2 (g) + H2O (l) 2) CaO (s) + CO2 (g) → CaCO3 (s) 3) Mg (s) + O2 (g) → MgO (s) 4) PbCO3 (s) → PbO (s) + CO2 (g) A) 1, 2, and 3 B) 1, 2, 3, and 4 C) 2 and 3 D) 4 only E) 2, 3, and 4 |
D
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The formula weight of potassium phosphate (K3PO4) is ________ u.
A) 173.17 B) 196.27 C) 212.27 D) 251.37 E) 86.07 |
C
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The mass % of C in methane (CH4) is ________.
A) 25.13 B) 74.87 C) 92.26 D) 133.6 E) 7.743 |
B
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The percentage by mass of nitrogen in PtCl2(NH3)
2 is ________ %N. A) 4.67 B) 4.95 C) 12.67 D) 9.34 E) 9.90 |
D
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One million argon atoms is ________ mol of argon atoms.
A) 1.7 × 10-18 B) 1.0 × 10-6 C) 1.0 × 10+6 D) 3 E) 6.0 × 1023 |
A
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A sample of CH2F2 with a mass of 19 g contains ________ atoms of F.
A) 2.2 × 1023 B) 4.4 × 1023 C) 9.5 D) 3.3 × 1024 E) 38 |
B
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There are ________ atoms of nitrogen are in 10 g of NH4NO3.
A) 1.8 B) 2 C) 1.5 × 1023 D) 3.0 × 1023 E) 3.5 |
C
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There are ________ moles of pyridine (C5H5N) contained in 3.13 g of pyridine.
A) 0.319 B) 0.00404 C) 0.0396 D) 25.3 E) 4.04 × 103 |
C
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The total number of atoms in 0.111 mol of Fe(CO)3(PH3)
2 is ________. A) 1.00 × 1024 B) 1.67 C) 2.76 × 10-24 D) 4.46 × 1021 E) 15 |
A
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