Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 73

Chloral hydrate $\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}_{3} \mathrm{O}_{2}\right)$ is a drug formerly used as a sedative and hypnotic. It is the compound used to make "Mickey Finns" in detective stories. a. Calculate the molar mass of chloral hydrate. b. What amount (moles) of $\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}_{3} \mathrm{O}_{2}\( molecules are in 500.0 \)\mathrm{g}$ chloral hydrate? c. What is the mass in grams of \(2.0 \times 10^{-2}\) mole of chloral hydrate? d. What number of chlorine atoms are in 5.0 g chloral hydrate? e. What mass of chloral hydrate would contain 1.0 g Cl? f. What is the mass of exactly 500 molecules of chloral hydrate?

Short Answer

Expert verified
a. The molar mass of chloral hydrate is 165.5 g/mol. b. There are approximately 3.021134 moles of chloral hydrate in 500.0 g of the compound. c. The mass of \(2.0 \times 10^{-2}\) mole of chloral hydrate is approximately 3.31 g. d. There are approximately \(5.46 \times 10^{22}\) chlorine atoms in 5.0 g of chloral hydrate. e. A mass of 1.554 g of chloral hydrate would contain 1.0 g of Cl. f. The mass of exactly 500 molecules of chloral hydrate is approximately \(1.373 \times 10^{-19}\) g.

Step by step solution

01

Molar mass of chloral hydrate

To calculate the molar mass of chloral hydrate, we first need to find the molar mass of each type of atom in its formula. The molar masses of carbon (C), hydrogen (H), chlorine (Cl), and oxygen (O) are approximately 12 g/mol, 1 g/mol, 35.5 g/mol, and 16 g/mol, respectively. The molar mass of chloral hydrate can be calculated as follows: Molar mass of chloral hydrate = (2 x 12) + (3 x 1) + (3 x 35.5) + (2 x 16) = 24 + 3 + 106.5 + 32 = 165.5 g/mol #b. What amount of moles of \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}_{3} \mathrm{O}_{2}\) molecules are in 500.0 \(\mathrm{g}\) chloral hydrate?#
02

Moles of chloral hydrate

To calculate the amount of moles of chloral hydrate, we can use the formula: moles = mass / molar mass moles = 500.0 g / 165.5 g/mol ≈ 3.021134 moles #c. What is the mass in grams of \(2.0 \times 10^{-2}\) mole of chloral hydrate?#
03

Mass of chloral hydrate

To find the mass of \(2.0 \times 10^{-2}\) mole of chloral hydrate, we can use the formula: mass = moles * molar mass mass = \(2.0 \times 10^{-2}\) mol * 165.5 g/mol ≈ 3.31 g #d. What number of chlorine atoms are in 5.0 g chloral hydrate?#
04

Chlorine atoms in chloral hydrate

First, we need to find the moles of chloral hydrate in 5.0 g: moles = mass / molar mass moles = 5.0 g / 165.5 g/mol ≈ 0.03021134 moles Since each mole of chloral hydrate contains 3 moles of chlorine atoms, the moles of chlorine atoms can be calculated as: moles of Cl = 0.03021134 moles * 3 = 0.09063402 moles Finally, we can find the number of chlorine atoms using Avogadro's number: \(\approx 6.022 \times 10^{23}\) atoms/mol: Number of Cl atoms = moles of Cl * Avogadro's number Number of Cl atoms ≈ 0.09063402 moles * 6.022 x 10^{23} atoms/mol ≈ 5.46 x 10^{22} atoms #e. What mass of chloral hydrate would contain 1.0 g Cl?#
05

Mass of chloral hydrate containing 1.0 g Cl

First, calculate the moles of Cl in 1.0 g: moles of Cl = mass / molar mass moles of Cl = 1.0 g / 35.5 g/mol ≈ 0.02816901 moles Since 3 moles of Cl are in one mole of chloral hydrate, we can find the moles of chloral hydrate as: moles of chloral hydrate = 0.02816901 moles / 3 = 0.00938967 moles Finally, calculate the mass of chloral hydrate containing such moles: mass = moles * molar mass mass = 0.00938967 moles * 165.5 g/mol ≈ 1.554 g #f. What is the mass of exactly 500 molecules of chloral hydrate?#
06

Mass of 500 molecules of chloral hydrate

First, convert 500 molecules to moles: moles = 500 molecules / 6.022 x 10^{23} molecules/mol ≈ 8.299699 x 10^{-22} moles Then, calculate the mass of these moles: mass = moles * molar mass mass = 8.299699 x 10^{-22} moles * 165.5 g/mol ≈ 1.373 x 10^{-19} g

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

A 9.780 -g gaseous mixture contains ethane $\left(\mathrm{C}_{2} \mathrm{H}_{6}\right)\( and propane \)\left(\mathrm{C}_{3} \mathrm{H}_{8}\right) .$ Complete combustion to form carbon dioxide and water requires 1.120 \(\mathrm{mole}\) of oxygen gas. Calculate the mass percent of ethane in the original mixture.

A \(2.25-\) g sample of scandium metal is reacted with excess hydrochloric acid to produce 0.1502 g hydrogen gas. What is the formula of the scandium chloride produced in the reaction?

A compound contains only carbon, hydrogen, nitrogen, and oxygen. Combustion of 0.157 \(\mathrm{g}\) of the compound produced 0.213 \(\mathrm{g} \mathrm{CO}_{2}\) and 0.0310 \(\mathrm{g} \mathrm{H}_{2} \mathrm{O}\) . In another experiment, it is found that 0.103 \(\mathrm{g}\) of the compound produces 0.0230 $\mathrm{g} \mathrm{NH}_{3} .$ What is the empirical formula of the compound? Hint: Combustion involves reacting with excess \(\mathrm{O}_{2}\) . Assume that all the carbon ends up in \(\mathrm{CO}_{2}\) and all the hydrogen ends up in \(\mathrm{H}_{2} \mathrm{O}\) . Also assume that all the nitrogen ends up in the \(\mathrm{NH}_{3}\) in the second experiment.

Balance the following equations: a. $\operatorname{Cr}(s)+\mathrm{S}_{8}(s) \rightarrow \mathrm{Cr}_{2} \mathrm{S}_{3}(s)$ b. \(\operatorname{NaHCO}_{3}(s) \stackrel{\mathrm{Heat}}{\longrightarrow}\) $\mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)$ c. \(\quad \mathrm{KClO}_{3}(s) \stackrel{\mathrm{Heat}}{\longrightarrow}\) \(\mathrm{KCl}(s)+\mathrm{O}_{2}(g)\) d. $\operatorname{Eu}(s)+\mathrm{HF}(g) \rightarrow \operatorname{EuF}_{3}(s)+\mathrm{H}_{2}(g)$

Tetrodotoxin is a toxic chemical found in fugu pufferfish, a popular but rare delicacy in Japan. This compound has an LD_s0 (the amount of substance that is lethal to \(50 . \%\) of a population sample) of \(10 . \mu \mathrm{g}\) per kg of body mass. Tetrodotoxin is 41.38\(\%\) carbon by mass, 13.16\(\%\) nitrogen by mass, and 5.37\(\%\) hydrogen by mass, with the remaining amount consisting of oxygen. What is the empirical formula of tetrodotoxin? If three molecules of tetrodotoxin have a mass of \(1.59 \times 10^{-21}\) g, what is the molecular formula of tetrodotoxin? What number of molecules of tetrodotoxin would be the LD_so dosage for a person weighing 165 \(\mathrm{lb}\) ?
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Making Measurements

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Ionic and Molecular Compounds

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free