Textbook Question
(b) In a desert, the temperature can be as high as 45 °C, what is the temperature in °F?
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Ch.1 - Introduction: Matter, Energy, and Measurement
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 1, Problem 36
(a) What is the mass of a silver cube whose edges measure 2.00 cm each at 25 _x001F_C? The density of silver is 10.49 g/cm3 at 25 _x001F_C. (b) The density of aluminum is 2.70 g/cm3 at 25 _x001F_C. What is the weight of the aluminum foil with an area of 0.5 m2 and a thickness of 0.5 mm?
Verified step by step guidance1
Calculate the volume of the silver cube using the formula for the volume of a cube: \( V = a^3 \), where \( a \) is the edge length of the cube. For a cube with edges of 2.00 cm, substitute the value into the formula.
Use the density formula \( \text{Density} = \frac{\text{Mass}}{\text{Volume}} \) to find the mass of the silver cube. Rearrange the formula to solve for mass: \( \text{Mass} = \text{Density} \times \text{Volume} \). Substitute the known values for density and volume.
Convert the area of the aluminum foil from square meters to square centimeters, as the density is given in g/cm³. Use the conversion factor: 1 m² = 10,000 cm².
Convert the thickness of the aluminum foil from millimeters to centimeters, as the density is given in g/cm³. Use the conversion factor: 1 mm = 0.1 cm.
Calculate the volume of the aluminum foil using the formula \( V = \text{Area} \times \text{Thickness} \). Then, use the density formula to find the mass: \( \text{Mass} = \text{Density} \times \text{Volume} \). Substitute the known values for density and volume.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Density
Density is defined as mass per unit volume, typically expressed in grams per cubic centimeter (g/cm³) in chemistry. It is a crucial property that helps determine how much mass is contained in a given volume of a substance. In this question, the densities of silver and aluminum are provided, which are essential for calculating the mass of the silver cube and the weight of the aluminum foil.
Recommended video:
Guided course
01:56
Density Concepts
Volume Calculation
To find the mass of an object using its density, one must first calculate its volume. For a cube, the volume is determined by cubing the length of one edge (V = edge³). In this case, the volume of the silver cube with edges measuring 2.00 cm must be calculated to find its mass using the given density.
Recommended video:
Guided course
02:35Constant-Volume Calorimetry
Weight Calculation
Weight is the force exerted by gravity on an object and can be calculated by multiplying the mass of the object by the acceleration due to gravity (W = mg). In the context of the aluminum foil, its mass can be derived from its volume (area × thickness) and density, allowing for the calculation of its weight in a straightforward manner.
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03:45Weight Conversion Example
Related Practice
Textbook Question
(b) Carbon dioxide (CO2) is a gas at room temperature and pressure. However, carbon dioxide can be put under pressure to become a 'supercritical fluid' that is a much safer dry-cleaning agent than tetrachloroethylene. At a certain pressure, the density of supercritical CO2 is 0.469 g/cm3. What is the mass of a 25.0-mL sample of supercritical CO2 at this pressure?
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Textbook Question
(c) Is a graduated cylinder such as that shown in Figure 1.21 likely to afford the accuracy of measurement needed?
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Textbook Question
(d) A cubic piece of metal measures 5.00 cm on each edge. If the metal is nickel, whose density is 8.90 g/cm3, what is the mass of the cube?
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Textbook Question
(a) A sample of tetrachloroethylene, a liquid used in dry cleaning that is being phased out because of its potential to cause cancer, has a mass of 40.55 g and a volume of 25.0 mL at 25 °C. What is its density at this temperature? Will tetrachloroethylene float on water? (Materials that are less dense than water will float.)
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Textbook Question
(b) An experiment requires 45.0 g of ethylene glycol, a liquid whose density is 1.114 g/mL. Rather than weigh the sample on a balance, a chemist chooses to dispense the liquid using a graduated cylinder. What volume of the liquid should he use?
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