Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 1: Problem 4

State whether the following statements are true or false. \(1 \mathrm{~g}\) atom of nitrogen contains \(6.023 \times 10^{23}\) atoms of nitrogen.

Short Answer

Expert verified
Answer: Yes, it is true that 1 gram atom of nitrogen contains \(6.023 \times 10^{23}\) atoms of nitrogen.

Step by step solution

01

Find the molar mass of nitrogen

To find out how many atoms are in 1 gram atom of nitrogen, we first need to know the molar mass of nitrogen. Nitrogen is a diatomic molecule with the formula N2. One atom of nitrogen has an atomic mass of 14.0067 u, so the molecular mass of N2 is twice the atomic mass of nitrogen: Molar mass of N2 = 2 × 14.0067 u = 28.0134 u
02

Convert 1 gram atom to moles

Next, we will convert the given 1 gram atom of nitrogen into moles. Since the molar mass of nitrogen is 28.0134 u: 1 gram atom of nitrogen = 1 × 28.0134 grams = 28.0134 grams Now, let's convert this mass into moles using the molar mass: Number of moles = (mass) / (molar mass) = (28.0134 grams) / (28.0134 g/mol) = 1 mole
03

Calculate the number of nitrogen atoms

Now that we have the number of moles, we can use Avogadro's number to find the number of nitrogen atoms: Number of nitrogen atoms = (number of moles) × (Avogadro's number) = (1 mole) × (\(6.023 \times 10^{23}\) atoms/mol) = \(6.023 \times 10^{23}\) atoms
04

Verify the statement

As we calculated, 1 gram atom of nitrogen contains \(6.023 \times 10^{23}\) atoms. Therefore, the given statement is true.

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

Select the correct alternative from the given choices. \(20 \mathrm{cc}\) of a hydrocarbon on complete combustion gave \(80 \mathrm{cc}\) of \(\mathrm{CO}_{2}\) and \(100 \mathrm{cc}\) of \(\mathrm{H}_{2} \mathrm{O}\) at \(\mathrm{STP}\). The empirical formula of that compound is (a) \(\mathrm{C}_{2} \mathrm{H}_{5}\) (b) \(\mathrm{C}_{2} \mathrm{H}_{6}\) (c) \(\mathrm{C}_{3} \mathrm{H}_{8}\) (d) \(\mathrm{C}_{4} \mathrm{H}_{10}\)

Arrange them in the ascending order of intermolecular forces of attraction. (a) \(\mathrm{C}, \mathrm{B}, \mathrm{D}, \mathrm{A}\) (b) \(\mathrm{A}, \mathrm{B}, \mathrm{C}, \mathrm{D}\) (c) \(\mathrm{D}, \mathrm{C}, \mathrm{B}, \mathrm{A}\) (d) A, C, B, D When ammonia gas is subjected to sudden expansion from a region of high pressure into a region of low pressure, which of the following changes is expected to take place? (a) decrease in kinetic energy and potential energy (b) conversion of kinetic energy to potential energy (c) conversion of potential energy to kinetic energy (d) increase in kinetic energy and potential energy

Calculate the molarity of a solution obtained by mixing \(250 \mathrm{ml}\) of \(0.5 \mathrm{M}\) HCl with \(750 \mathrm{ml}\) of \(2 \mathrm{M}\) HCl. (a) \(1.8\) (b) \(2.0\) (c) \(1.6\) (d) \(0.8\)

A certain mass of a gas occupies a volume of 600 \(\mathrm{ml}\) at a certain temperature and pressure. If pressure is decreased by \(40 \%\) what will be the volume occupied by the same mass of the gas at the same temperature? (a) \(240 \mathrm{ml}\) (b) \(1000 \mathrm{ml}\) (c) \(300 \mathrm{ml}\) (d) \(120 \mathrm{ml}\)

State whether the following statements are true or false. Gases show deviations from ideal behaviour at high temperatures and high pressures.
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Kinetics

Read Explanation

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

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