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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Ch.1 - Introduction: Matter, Energy, and Measurement
Chapter 1, Problem 38b
(b) An experiment requires 15.0 g of cyclohexane, whose density at 25 C is 0.7781 g>mL. What volume of cyclohexane should be used?
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Identify the given values: mass of cyclohexane = 15.0 g and density of cyclohexane = 0.7781 g/mL.
Recall the formula for density: \( \text{Density} = \frac{\text{Mass}}{\text{Volume}} \).
Rearrange the formula to solve for volume: \( \text{Volume} = \frac{\text{Mass}}{\text{Density}} \).
Substitute the given values into the rearranged formula: \( \text{Volume} = \frac{15.0 \text{ g}}{0.7781 \text{ g/mL}} \).
Calculate the volume to find out how many milliliters of cyclohexane are needed.
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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 milliliter (g/mL) or kilograms per cubic meter (kg/m³). It is a crucial property of substances that helps in determining how much space a given mass of material occupies. In this question, the density of cyclohexane is provided, which allows us to calculate its volume based on the mass given.
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Density Concepts
Volume Calculation
Volume can be calculated using the formula: Volume = Mass / Density. This relationship shows how mass and density are inversely related; as density increases, the volume for a given mass decreases. In the context of the question, knowing the mass of cyclohexane and its density enables us to find the required volume for the experiment.
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Units of Measurement
Understanding units of measurement is essential in chemistry, as it ensures that calculations are accurate and meaningful. In this question, mass is given in grams, density in grams per milliliter, and the resulting volume will be in milliliters. Properly converting and using these units is vital for obtaining the correct volume of cyclohexane needed for the experiment.
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Related Practice
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) After the label fell off a bottle containing a clear liquid believed to be benzene, a chemist measured the density of the liquid to verify its identity. A 25.0-mL portion of the liquid had a mass of 21.95 g. A chemistry handbook lists the density of benzene at 15 °C as 0.8787 g/mL. Is the calculated density in agreement with the tabulated value?
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Textbook Question
(c) A spherical ball of lead has a diameter of 5.0 cm. What is the mass of the sphere if lead has a density of 11.34 g>cm3? (The volume of a sphere is 14>32pr3, where r is the radius.)
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Textbook Question
If on a certain year, an estimated amount of 4 million metrictons (1 metric ton = 1000 kg) of nitrous oxide 1N2O2 wasemitted worldwide due to agricultural activities, express thismass of N2O in grams without exponential notation, usingan appropriate metric prefix.
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Textbook Question
Use of the British thermal unit (Btu) is common in some types of engineering work. A Btu is the amount of heat required to raise the temperature of 1 lb of water by 1°F. Calculate the number of joules in a Btu.
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