CHEM101 (E-1) Chemistry I - Eastwick College
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Free CHEM101 (E-1) Chemistry I - Eastwick College Questions
643 g ÷ 19.3 g/mL = 0.137 mL.
- If 15.0 mL of a metal has a mass of 103.0 g, what is the density of the metal?
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1.46 g/mL
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0.146 g/mL
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1550 g/mL
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9.867 g/mL
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6.87 g/mL
Explanation
Correct Answer: (E) 6.87 g/mL
Density is calculated using the formula: Density = Mass ÷ Volume
103.0 g ÷ 15.0 mL = 6.87 g/mL
0 g ÷ 15.0 mL = 6.87 g/mL
- Which of these is the correct normal decimal notation for 5.23 × 10⁻⁴?
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52,300
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0.00523
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0.000523
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0.0523
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0.0000523
Explanation
Correct Answer: (C) 0.000523
To convert from scientific notation to decimal notation, move the decimal point to the left by the number of places indicated by the negative exponent. Since the exponent is −4, the decimal point moves 4 places to the left:
5.23 × 10⁻⁴ = 0.000523
23 × 10⁻⁴ = 0.000523
- Determine the density of a 100.0 g sample of mercury having a volume of 7.36 cm³. Carry out the calculation to the correct number of significant digits.
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183 g/cm³
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0.0732 g/cm³
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0.073 g/cm³
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13.58 g/cm³
-
13.66 g/cm³
Explanation
Correct Answer: (D) 13.58 g/cm³
Density = Mass ÷ Volume
0 g ÷ 7.36 cm³ = 13.586... g/cm³
- 7.85 × 10⁴ kg
- 1.1 kg
- 78.54 kg
- 1.1 × 10² kg
- 3.8 × 10⁵ kg
Explanation
Correct Answer: (C) 78.54 kg
First convert pounds to grams: 173 lb × 454 g/lb = 78,542 g
Then convert grams to kilograms: 78,542 g ÷ 1000 = 78.54 kg.
0 g ÷ 3.66 mL = 13.66 g/mL
The answer is expressed to 4 significant figures, consistent with the given values of 50.0 g (3 sig figs) and 3.66 mL (3 sig figs), giving a result of 13.7 g/mL to 3 significant figures. Among the answer choices, 13.66 g/mL is the most accurate result of the calculation.
- How many protons (p), neutrons (n), and electrons (e) are in an atom of ²³⁵U?
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92 p, 92 n, 146 e
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92 p, 146 n, 92 e
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92 p, 51 n, 92 e
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92 p, 92 n, 92 e
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92 p, 143 n, 92 e
Explanation
Correct Answer: (E) 92 p, 143 n, 92 e
Uranium (U) has an atomic number of 92, which means it has 92 protons. In a neutral atom, the number of electrons equals the number of protons, so there are also 92 electrons. The mass number of 235 represents the total number of protons and neutrons, so the number of neutrons is calculated as:
235 − 92 = 143 neutrons
- Compound
- Ion
- Nucleus
- Element
- Mixture
Explanation
Correct Answer: (D) Element
An element is the simplest form of a substance that cannot be broken down into simpler substances by ordinary chemical means. Each element is made up of only one type of atom and is represented on the periodic table. Elements are the fundamental building blocks of all matter.
Why the other options are incorrect:
A. Compound – A compound is formed when two or more elements are chemically combined in fixed proportions. It is more complex than an element, not simpler.
B. Ion – An ion is an atom or group of atoms that has gained or lost electrons, giving it a positive or negative charge. It is not the simplest form of a substance.
C. Nucleus – The nucleus is the central part of an atom containing protons and neutrons. It is a component of an atom, not a form of a substance.
E. Mixture – A mixture consists of two or more substances physically combined without a fixed ratio. It is more complex than an element.
5 m × 1000 mm/m = 89,500 mm = 8.95 × 10⁴ mm
- Which of these is the correct scientific notation for 6,000,220?
-
6.00022 × 10⁶
-
6.00022 × 10⁻⁵
-
6.00022 × 10⁻⁶
-
6.00022 × 10⁵
-
6.022 × 10⁶
Explanation
Correct Answer: (A) The pH of the solution rises significantly when the volume of the base is increased from 14 mL to 18 mL.
Based on the graph in Figure 2-1, the pH remains relatively low and stable from approximately 2 to 14 mL of base addition. However, between approximately 14 mL and 18 mL there is a sharp and dramatic increase in pH, rising from around 4-5 to approximately 9. This steep rise is characteristic of the equivalence point region in an acid-base titration curve.
Why the other options are incorrect:
B. The pH of the solution must be determined algebraically. — The graph directly provides pH values visually at each volume of base added. Algebraic determination is not required to read the data from the graph.
C. The pH of the solution is relatively constant after the addition of the first 14 mL of the base. — The graph shows that pH is relatively constant before 14 mL, not after. After 14 mL, the pH rises sharply.
D. The pH of the solution is relatively unaffected by the addition of the base. — This is clearly incorrect as the graph shows a dramatic pH increase between 14 mL and 18 mL of base addition.
E. The pH of the solution is 7 when approximately 16 mL of the base has been added. — According to the graph, at approximately 16 mL the pH is in the steep rise region and is closer to 7-8, but the graph shows pH reaching approximately 7 closer to the midpoint of the steep rise rather than a clearly defined point at exactly 16 mL. The more clearly supported observation from the graph is the significant rise between 14 and 18 mL.
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