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Ch.1 - Introduction: Matter, Energy, and Measurement
Chapter 1, Problem 35b

(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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1
Identify the given values: density of supercritical CO_2 is 0.469 g/cm^3 and the volume of the sample is 25.0 mL.
Recall the formula for mass using density and volume: mass=density×volume.
Substitute the given values into the formula: mass=0.469g/cm3×25.0mL.
Note that 1 mL is equivalent to 1 cm^3, so the units are consistent and will cancel appropriately.
Perform the multiplication to find the mass of the supercritical CO_2 sample.

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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 cubic centimeter (g/cm³). It is a crucial property that helps determine how much mass is contained in a given volume of a substance. In this question, the density of supercritical CO₂ is provided, allowing us to calculate the mass of a specific volume of the substance.
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Supercritical Fluids

Supercritical fluids occur when a substance is subjected to temperature and pressure above its critical point, resulting in unique properties that are distinct from gases and liquids. Supercritical CO₂, for example, can dissolve materials like a liquid while maintaining the diffusivity of a gas, making it useful in applications such as dry cleaning. Understanding this concept is essential for grasping the context of the question.
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Mass Calculation

Mass calculation involves using the formula mass = density × volume. In this scenario, knowing the density of supercritical CO₂ and the volume of the sample allows us to compute the mass. This fundamental relationship is key to solving the problem presented in the question.
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Related Practice
Textbook Question

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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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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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Open Question
(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?
Textbook Question

(a) To identify a liquid substance, a student determined its density. Using a graduated cylinder, she measured out a 45-mL sample of the substance. She then measured the mass of the sample, finding that it weighed 38.5 g. She knew that the substance had to be either isopropyl alcohol 1density 0.785 g/mL2 or toluene (density 0.866 g/mL). What are the calculated density and the probable identity of the substance?

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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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