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1. Intro to General Chemistry

**Density** represents the mass of an object or compound within a given volume.

Understanding Density

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so density represents the amount of mass per unit of volume. And here we have our purple box again. Remember, when we have a purple box, that means that is a formula or some type of concept you need to commit to memory. So density is equal to mass over volume. Depending on the phase of matter, the units Ford can be different. So we're gonna say for solids and liquids which are more dense than gasses, solids and liquids have the unit for mass in grams and a unit for volume in middle leaders. Or they have the unit for mass still in grams or the units for volume in Centimeters Cube. Remember when we talked about conversion factors for volume? We said that one middle leader was equal toe one centimeters. Cute. That's why we're allowed to basically swap out MLS here for centimeters cubes here. Now, gasses themselves are much less dense than solids and liquids, so their units for density are a little bit different, their masses still Ingram's. But now, because they're less dense, we wouldn't use milliliters, would use leaders and remember within our conversion factors. We said that one mil on one leader was equal toe one Desa meters cute. So we could say the density of gas is is grams per leader or grams per desa meters cute. So just remember, density itself is just massive volume. Depending on the face of matter that we're dealing with, the units can be slightly different. Now that we've looked at the basic set up of density, let's move on to our example and practice questions.

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So here in this example question, it says if the density of an unknown metal is 21.4 g per centimeters, cube express its density in pounds per feet. Cute. Alright. So here that the information they're giving to us is not a given amount. It's actually a conversion factor. It's 21.4 g per one centimeters cute, and they're telling us that we need to get to our end amounts, which will be pounds per feet. Cute. We can set this up as a dimensional analysis type of question because all we're doing is setting things up with conversion factors, allowing them to cancel out and wind up with end units or end amounts. All right, so we need to find a way of changing grams to pounds and changing Centimeters Cube to feed. Cute. So let's do the easier one first. Let's go from grams to pounds here. We're going to use a new conversion factor. Where would he starting out with our first conversion factor? This question actually doesn't have a given amount. Ah, unit by itself. That can happen now. We know that there is a connection between grams and pounds when We talked about the different types of conversion factors. We said here that £1 was equal to 453.59 g grams go on the bottom so that they can cancel out like this. So we've done the easy part. We've converted grams to pounds. Now it's up to us to convert Centimeters Cube 2 ft. Cute. All right, So what we're gonna do first is we're going to say that there is a connection between centimeters and inches. We want to get rid of these centimeters, which are on the bottom. So we actually have to put centimeters here on top. Centimeters and inches air connected, and the relationship is that one inch is equal to 2. centimeters. However, this is cube, and these centimeters here are not. So you would cube the whole thing. We'll come back and see what effect that has on our numbers. So basically, centimeters cubes or cancel out. Now we have inches cube. We want to get rid of inches, so we put inches up here. We want feet. Remember, there's a connection between ancient feet, and that's 1 ft is equal to 12 inches, these inches air cubed. But these air Not so I'd have to cute this whole thing, and this would represent my conversion factor for inches. Cancel out in just cubes. Cancel out. So what I'd have at the end is pounds over Feet Cube. Which of the units I'm trying to isolate. Let's come down here and see what effect with all of this. Have so we have 21.4 g, and then we have on the bottom one centimeters Cube. We'd have £1 for 4 53. g when we do. 2.54 cube. That's 2.54 times 2.54 times 2. That comes out to 16. centimeters. Cube over one cube is just one over inches. Cube and then 12 cube is 12 times 12 times 12, which is 17 28 inches. Cube over 1 ft cube. So conversion factor and four Counseling. All the units will give us what we need for end amount, which will be in pounds per feet. Cube. If we look, it would be 21.4 times 16.387 times 17 28 divided on the bottom by 453.59 So we get initially is we would get 35.97 But remember the number of sick fixing your your answer is based on the digits given within the question 21.4 has within it three significant figures. So our answer needs three significant figures. To get that, I'd have to convert it to scientific notation. So I go 123 spaces, and this will come out to be 1.34 times 10 to the three pounds per feet cube as our final answer. So this would be a way of converting the units of density from one set of values toe another set of values. Remember, it's treated like a dimensional analysis question. Use conversion factors in orderto isolate your and amounts at the end. It just happens to be here that are end amounts are two units those of pounds and feet cube

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Problem

When lead levels in blood exceed 0.80 ppm (parts per million) the level is considered dangerous. 0.80 ppm means that 1 million g of blood would contain 0.80 g of Pb. Given that the density of blood is 1.060 kg/cm^{3}, how many grams of Pb would be found in 400.00 mL of blood at 0.620 ppm?

A

0.891 g Pb

B

0.522 g Pb

C

0.263 g Pb

D

0.059 g Pb

Additional resources for Density

PRACTICE PROBLEMS AND ACTIVITIES (41)

- Consider the two spheres shown here, one made of silver and the other of aluminum. (a) What is the mass of eac...
- Consider the two spheres shown here, one made of silver and the other of aluminum. (a) What is the mass of eac...
- (b) Three cubes of equal mass are composed of gold 1density = 19.32 g/cm32, platinum 1density = 21.45 g/cm32, ...
- Consider 20 mL samples of the following liquids. Which sample has the largest mass? (LO 1.9) (a) Water (densi...
- The cylinder contains two liquids that do not mix with one another: water (density = 1.0 g/mL) and vegetable o...
- Which block in each of the following drawings of a balance is more dense, red or green? Explain.
- The following cylinder contains three liquids that do not mix with one another: water (density = 1.0 g/mL), ve...
- (b) Carbon dioxide 1CO22 is a gas at room temperature and pressure. However, carbon dioxide can be put under p...
- (a) A sample of tetrachloroethylene, a liquid used in dry cleaning that is being phased out because of its pot...
- (b) An experiment requires 45.0 g of ethylene glycol, a liquid whose density is 1.114 g>mL. Rather than wei...
- (a) To identify a liquid substance, a student determined its density. Using a graduated cylinder, she measured...
- (b) An experiment requires 15.0 g of cyclohexane, whose density at 25 C is 0.7781 g>mL. What volume of cycl...
- (a) After the label fell off a bottle containing a clear liquid believed to be benzene, a chemist measured the...
- The density of air at ordinary atmospheric pressure and 25 C is 1.19 g/L. What is the mass, in kilograms, of t...
- A new penny has a mass of 2.49 g and a volume of 0.349 cm3. Is the penny made of pure copper? Explain your ans...
- What is the density of glass in g/cm3 if a sample weighing 27.43 g has a volume of 12.40 cm3?
- What is the density of lead in g/cm3 if a sample weighing 206.77 g has a volume of 15.50 cm3?
- Glycerol is a syrupy liquid often used in cosmetics and soaps. A 3.25 L sample of pure glycerol has a mass of ...
- A vessel contains 4.67 L of bromine whose density is 3.10 g/cm3. What is the mass of the bromine in the vessel...
- Ethylene glycol (antifreeze) has a density of 1.11 g>cm3. a. What is the mass in g of 417 mL of ethylene gl...
- Aspirin has a density of 1.40 g/cm3. What is the volume in cubic centimeters of an aspirin tablet weighing 250...
- Ethylene glycol (antifreeze) has a density of 1.11 g>cm3. a. What is the mass in g of 417 mL of ethylene gl...
- Gaseous hydrogen has a density of 0.0899 g/L at 0 °C, and gaseous chlorine has a density of 3.214 g/L at the s...
- Acetone (nail polish remover) has a density of 0.7857 g>cm3. a. What is the mass in g of 28.56 mL of aceto...
- A small airplane takes on 245 L of fuel. If the density of the fuel is 0.821 g>mL, what mass of fuel has th...
- Human fat has a density of 0.918 g>cm3. How much volume (in cm3) is gained by a person who gains 10.0 lb o...
- The density of chloroform, a widely used organic solvent, is 1.4832 g/mL at 20 °C. How many milliliters would ...
- More sulfuric acid (density = 1.8302 g/cm3) is produced than any other chemical—approximately 3.6 * 1011 lb/yr...
- Two spheres of equal volume are placed on the scales as shown. Which one is more dense?
- Water has a density of 0.997 g>cm3 at 25 C; ice has a density of 0.917 g>cm3 at -10 C. (a) If a soft-dri...
- A flask containing 11.7 mL of a liquid weighs 132.8 g with the liquid in the flask and 124.1 g when empty. Cal...
- Gold is alloyed (mixed) with other metals to increase its hardness in making jewelry. (b) The relative amount ...
- You are assigned the task of separating a desired granular material with a density of 3.62 g>cm3 from an un...
- When an irregularly shaped chunk of silicon weighing 8.763 g was placed in a graduated cylinder containing 25....
- Answer the following questions. (d) A particular sample of crude oil has a density of 0.85 g/mL. What is the m...
- Answer the following questions. (c) A certain type of wood has a density of 0.40 g/cm3. What is the mass of 1....
- A bag of Hershey’s Kisses contains the following information: Serving size: 9 pieces = 41 g Calories per servi...
- Vinaigrette salad dressing consists mainly of oil and vinegar. The density of olive oil is 0.918 g/cm3, the de...
- A calibrated flask was filled to the 25.00 mL mark with ethyl alcohol. By weighing the flask before and after ...
- The density of titanium is 4.51 g>cm3. What is the volume (in cubic inches) of 3.5 lb of titanium?
- An iceberg has a volume of 7655 ft2. What is the mass of the ice (in kg) composing the iceberg (at 0 °C)?

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