Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 13: Problem 29

Find the mass (in \(\mathrm{kg}\) ) of one molecule of \(\mathrm{CO}_{2}\)

Short Answer

Expert verified
Answer: The mass of one CO2 molecule is approximately \(7.310 \times 10^{-26} kg\).

Step by step solution

01

Find the molar mass of CO2

To find the molar mass of CO2, we need to know the molar mass of each element and their respective number of atoms in a CO2 molecule. A CO2 molecule is composed of one carbon (C) atom and two oxygen (O) atoms. The molar mass of carbon is 12.01 g/mol, and the molar mass of oxygen is 16.00 g/mol. To find the molar mass of CO2, multiply the molar mass of each element by the number of its atoms in the molecule and then add the results: Molar mass of CO2 = (1 × 12.01 g/mol) + (2 × 16.00 g/mol) = 12.01 g/mol + 32.00 g/mol = 44.01 g/mol.
02

Convert g/mol to kg/mol

Since we need to find the mass in kg, we first need to convert the molar mass from grams to kilograms. We know that 1 kg = 1000 g, so divide the molar mass by 1000: Molar mass of CO2 = 44.01 g/mol ÷ 1000 = 0.04401 kg/mol.
03

Use Avogadro's number to find the mass of one molecule

Now, we'll use Avogadro's number (6.022 × 10^{23} ) to find the mass of a single CO2 molecule. Since there are 6.022 × 10^{23} molecules in a mole, we can divide the molar mass by Avogadro's number to find the mass of one molecule: Mass of one CO2 molecule = \(\frac{0.04401 kg/mol}{6.022 \times 10^{23} molecules/mol}\).
04

Calculate the mass of one molecule

Now, you can perform the operation to find the mass of a single CO2 molecule: Mass of one CO2 molecule = \(\frac{0.04401 kg/mol}{6.022 \times 10^{23} molecules/mol} \approx 7.310 \times 10^{-26} kg\). So, the mass of one CO2 molecule is approximately \(7.310 \times 10^{-26} kg\).

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

The SR- 71 Blackbird reconnaissance aircraft is primarily made of titanium and typically flies at speeds above Mach \(3 .\) In flight, the length of the SR- 71 increases by about \(0.20 \mathrm{m}\) from its takeoff length of $32.70 \mathrm{m} .$ The average coefficient of linear expansion for titanium over the temperature range experienced by the \(\mathrm{SR}-71\) is $10.1 \times 10^{-6} \mathrm{K}^{-1} .$ What is the approximate temperature of the SR-71 while it is in flight if it started at \(20^{\circ} \mathrm{C} ?\)
A scuba diver has an air tank with a volume of \(0.010 \mathrm{m}^{3}\) The air in the tank is initially at a pressure of \(1.0 \times 10^{7} \mathrm{Pa}\) Assuming that the diver breathes \(0.500 \mathrm{L} / \mathrm{s}\) of air, find how long the tank will last at depths of (a) \(2.0 \mathrm{m}\) and (b) $20.0 \mathrm{m} .\( (Make the same assumptions as in Example \)13.6 .)$
A hydrogen balloon at Earth's surface has a volume of \(5.0 \mathrm{m}^{3}\) on a day when the temperature is \(27^{\circ} \mathrm{C}\) and the pressure is \(1.00 \times 10^{5} \mathrm{N} / \mathrm{m}^{2} .\) The balloon rises and expands as the pressure drops. What would the volume of the same number of moles of hydrogen be at an altitude of \(40 \mathrm{km}\) where the pressure is \(0.33 \times 10^{3} \mathrm{N} / \mathrm{m}^{2}\) and the temperature is \(-13^{\circ} \mathrm{C} ?\)
If the upper atmosphere of Jupiter has a temperature of \(160 \mathrm{K}\) and the escape speed is \(60 \mathrm{km} / \mathrm{s}\), would an astronaut expect to find much hydrogen there?
A hand pump is being used to inflate a bicycle tire that has a gauge pressure of 40.0 psi. If the pump is a cylinder of length 18.0 in. with a cross- sectional area of 3.00 in. \(^{2},\) how far down must the piston be pushed before air will flow into the tire?
See all solutions

Recommended explanations on Physics Textbooks

Work Energy and Power

Read Explanation

Electrostatics

Read Explanation

Dynamics

Read Explanation

Famous Physicists

Read Explanation

Energy Physics

Read Explanation

Physics of Motion

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