Skip to main content
Pearson+ LogoPearson+ Logo
Ch.1 - Introduction: Matter, Energy, and Measurement
Back
Previous problem
Next problem
All textbooksBrown 14th EditionCh.1 - Introduction: Matter, Energy, and MeasurementProblem 37b

Chapter 1, Problem 37b

(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?

Verified Solution
Video duration:
1m
This video solution was recommended by our tutors as helpful for the problem above.
1037
views
Was this helpful?

Video transcript

Hi everyone today, we have a question telling us that a chemical reaction for an experiment needs 53. g of painting. However, the balance in the lab was taken for maintenance and is therefore unavailable. It was decided to use a pipette to measure the painting, calculate the volume needed if the density of plantain is 0.6-6 g per milliliter. So we're going to use the formula density equals mass over volume, and we want to solve for volume. So volume is going to equal mass, divided by density and now plugging in what we know. Our volume Is going to equal 53 0.4 g, divided by zero . ml Which equals .3 Mil leaders. And that is our final answer. Thank you for watching. Bye.
Previous problemNext problem
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.)

1302
views
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
views
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?

1320
views
Textbook Question

(c) Is a graduated cylinder such as that shown in Figure 1.21 likely to afford the accuracy of measurement needed?

634
views
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?

1450
views
1
rank
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?

850
views