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

Chapter 1, Problem 37c

(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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Hi everyone for this problem. It reads a graduated pipette is shown in the figure below. Can it afford to measure 15.2 ml of sample accurately? Alright, so looking at our graduated pipette below, we see by looking here that it has one mil leader markings. Okay. And with these one millimeter markings, we can measure the volume with uncertainty to the nearest millimeter and estimate 10th of a millimeter. So looking at the volume that's given, were given 15.2 mL and it has an uncertainty to the 10th place. So a graduated pipette can afford to measure 15. mL of sample accurately. Answer for this problem is going to be yes because like we said, we looked at the the one male leader markings and we can measure the volume with uncertainty to the nearest male leader and estimate 10th of a male leader. And this 15.2 has a tense. It can afford to measure it because it has uncertainty to the 10th place. So our final answer is going to be yes for this question. And that is it for this problem. I hope this was helpful
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(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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(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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(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?

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Textbook Question

(b) An experiment requires 15.0 g of cyclohexane, whose density at 25 C is 0.7781 g>mL. What volume of cyclohexane should be used?

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