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
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.
Related Practice
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) 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
(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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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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