/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 29 Pheromones are a special type of... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 3: Problem 29

Pheromones are a special type of compound secreted by the females of many insect species to attract the males for mating. One pheromone has the molecular formula \(\mathrm{C}_{19} \mathrm{H}_{38} \mathrm{O}\). Normally, the amount of this pheromone secreted by a female insect is about \(1.0 \times 10^{-12} \mathrm{~g} .\) How many molecules are there in this quantity?

Short Answer

Expert verified
The number of molecules in \(1.0 \times 10^{-12} \, \mathrm{g}\) of the pheromone \(\mathrm{C}_{19} \mathrm{H}_{38} \mathrm{O}\) is approximately \(2.295 \times 10^9\).

Step by step solution

01

Calculate the Molecular Mass

Firstly, get the molecular mass for \(\mathrm{C}_{19} \mathrm{H}_{38} \mathrm{O}\). The atomic masses of Carbon (C), Hydrogen (H), and Oxygen (O) are approximately 12 g/mol, 1 g/mol, and 16 g/mol respectively. The molecular mass is the sum of the atomic masses (19C + 38H + 1O) which equals \(19\times12 + 38\times1 + 16 = 262 \, \mathrm{g/mol}\).
02

Convert mass in grams to moles

Secondly, convert the given mass of the pheromone from grams to moles. The formula required is: \[\text{Moles} = \frac{\text{Mass (in g)}}{\text{Molar mass (in g/mol)}}\]Hence, moles of the substance is: \[\frac{1.0 \times 10^{-12} \, \mathrm{g}}{262 \, \mathrm{g/mol}} = 3.816 \times 10^{-15} \, \mathrm{mol}\]
03

Calculate the number of molecules

Lastly, calculate the number of molecules using Avogadro's number, which gives the number of entities in one mole. The formula required is: \[\text{Number of molecules} = \text{Moles} \times \text{Avogadro's number}\]Therefore, the number of molecules is: \[3.816 \times 10^{-15} \, \mathrm{mol} \times 6.022 \times 10^{23} \, \mathrm{mol^{-1}} = 2.295 \times 10^9 \, \mathrm{molecules}\]

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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

How many moles of cobalt (Co) atoms are there in \(6.00 \times 10^{9}(6\) billion) Co atoms?

Potash is any potassium mineral that is used for its potassium content. Most of the potash produced in the United States goes into fertilizer. The major sources of potash are potassium chloride \((\mathrm{KCl})\) and potassium sulfate \(\left(\mathrm{K}_{2} \mathrm{SO}_{4}\right)\). Potash production is often reported as the potassium oxide \(\left(\mathrm{K}_{2} \mathrm{O}\right)\) equivalent or the amount of \(\mathrm{K}_{2} \mathrm{O}\) that could be made from a given mineral. (a) If \(\mathrm{KCl}\) costs \(\$ 0.055\) per \(\mathrm{kg}\), for what price (dollar per \(\mathrm{kg}\) ) must \(\mathrm{K}_{2} \mathrm{SO}_{4}\) be sold in order to supply the same amount of potassium on a per dollar basis? (b) What mass (in \(\mathrm{kg}\) ) of \(\mathrm{K}_{2} \mathrm{O}\) contains the same number of moles of \(\mathrm{K}\) atoms as \(1.00 \mathrm{~kg}\) of \(\mathrm{KCl} ?\)

When baking soda (sodium bicarbonate or sodium hydrogen carbonate, \(\mathrm{NaHCO}_{3}\) ) is heated, it releases carbon dioxide gas, which is responsible for the rising of cookies, donuts, and bread. (a) Write a balanced equation for the decomposition of the compound (one of the products is \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) ). (b) Calculate the mass of \(\mathrm{NaHCO}_{3}\) required to produce \(20.5 \mathrm{~g}\) of \(\mathrm{CO}_{2.}\)

A sample of a compound of \(\mathrm{Cl}\) and \(\mathrm{O}\) reacts with an excess of \(\mathrm{H}_{2}\) to give \(0.233 \mathrm{~g}\) of \(\mathrm{HCl}\) and \(0.403 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}\). Determine the empirical formula of the compound.

The formula for rust can be represented by \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) How many moles of Fe are present in \(24.6 \mathrm{~g}\) of the compound?
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Organic Chemistry

Read Explanation

Kinetics

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.