Ch.1 - Introduction: Matter, Energy, and Measurement

Brown - Chemistry: The Central Science 15th Edition

Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook

Brown 15th Edition

Ch.1 - Introduction: Matter, Energy, and Measurement

Problem 39b

Chapter 1, Problem 39b

b. An experiment requires 78.1 g of benzene, a liquid whose density is 0.876 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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Identify the given values: mass of benzene (78.1 g) and density of benzene (0.876 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: \( \text{Volume} = \frac{78.1 \text{ g}}{0.876 \text{ g/mL}} \).

Calculate the volume to determine how much benzene to dispense using the graduated cylinder.

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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 the mass of a substance per unit volume, typically expressed in grams per milliliter (g/mL) for liquids. It is a crucial property that helps determine how much space a given mass of a substance will occupy. In this case, the density of benzene (0.876 g/mL) allows the chemist to convert the mass of benzene (78.1 g) into volume using the formula: Volume = Mass / Density.

Volume Calculation

Volume calculation involves determining the amount of three-dimensional space an object or substance occupies. For liquids, this is often measured in milliliters (mL). To find the volume of benzene needed for the experiment, the chemist will use the rearranged density formula, which allows for the calculation of volume based on the known mass and density of the liquid.

Graduated Cylinder Usage

A graduated cylinder is a common laboratory instrument used to measure the volume of liquids accurately. It is marked with a scale that allows for precise readings. In this scenario, the chemist will use the calculated volume of benzene to fill the graduated cylinder to the appropriate mark, ensuring that the correct amount of liquid is dispensed for the experiment.

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Textbook Question

a. After the label fell off a bottle containing a clear liquid believed to be a solvent called tetrahydrofuran, a chemist measured the density of the liquid to verify its identity. A 25.0-mL portion of the liquid had a mass of 22.08 g. A chemistry handbook lists the density of tetrahydrofuran at 25 °C as 0.8833 g/mL. Is the calculated density in agreement with the tabulated value?

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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?

1664

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Textbook Question

Many scientific data are reported at 25 °C. What is this temperature in kelvins and in degrees Fahrenheit?

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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?

(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

c. 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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