/*! 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 86 The percentage by weight of hydr... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 15: Problem 86

The percentage by weight of hydrogen in \(\mathrm{H}_{2} \mathrm{O}_{2}\) is (a) \(6.5\) (b) \(5.88\) (c) 25 (d) 50

Short Answer

Expert verified
The percentage by weight of hydrogen in \(\mathrm{H}_2\mathrm{O}_2\) is (b) \(5.88\).

Step by step solution

01

Determine the molar mass of hydrogen peroxide

First, find the molecular formula of hydrogen peroxide, which is \( \text{H}_2 \text{O}_2 \). To calculate the molar mass, add the atomic masses of all the atoms present: Hydrogen (H) has an atomic mass of approximately 1 g/mol and Oxygen (O) has an atomic mass of approximately 16 g/mol. Therefore, the molar mass of hydrogen peroxide is: \[ 2 \times 1 + 2 \times 16 = 2 + 32 = 34 \text{ g/mol} \]
02

Calculate the contribution of hydrogen to the molar mass

Since there are two hydrogen atoms in hydrogen peroxide and each has a mass of approximately 1 g/mol, the contribution of hydrogen to the total molar mass is: \[ 2 \times 1 = 2 \text{ g/mol} \]
03

Find the percentage by weight of hydrogen

To find the percentage by weight, divide the total mass of hydrogen by the molar mass of the compound and multiply by 100: \[ \frac{2}{34} \times 100 \approx 5.88 \% \]
04

Choose the correct option

The calculated percentage by weight of hydrogen in hydrogen peroxide is approximately 5.88%. Therefore, the correct option is (b) \(5.88\).

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!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Molar Mass Calculation
The molar mass of a substance is the mass of one mole of that substance in grams. It takes into account all the atoms that make up a molecule. To find it, you need to sum the atomic masses of each element in the compound. For instance, calculating the molar mass of hydrogen peroxide (H鈧侽鈧�) requires you to know the atomic masses of hydrogen (H) and oxygen (O).
  • Hydrogen has an atomic mass of approximately 1 g/mol.
  • Oxygen has an atomic mass of approximately 16 g/mol.
To find the total molar mass, add together the contribution of all atoms:\[ 2 \times (1 \text{ g/mol}) + 2 \times (16 \text{ g/mol}) = 34 \text{ g/mol} \]Understanding molar mass is crucial because it lets you determine how much of each element is present in a mole of the compound.
Atomic Mass
Atomic mass is the mass of a single atom of a chemical element, often expressed in atomic mass units (amu). Each element has a unique atomic mass, which is found on the periodic table. Atomic mass helps determine how much each element contributes to a compound's molar mass. For example, in hydrogen peroxide (H鈧侽鈧�):
  • Hydrogen contributes approximately 1 g/mol for each atom.
  • Oxygen contributes approximately 16 g/mol for each atom.
With this information, one can determine how each element's atomic mass contributes to the overall composition of the compound.
Molecular Formula
The molecular formula of a compound indicates the actual number of each type of atom present in a molecule. It provides critical information that allows you to calculate the molar mass. For hydrogen peroxide (H鈧侽鈧�), the formula reveals there are:
  • 2 hydrogen atoms
  • 2 oxygen atoms
This is fundamental because knowing the molecular formula helps in calculating percentages and understanding the compound's properties. Once you know the molecular formula, you can proceed to perform calculations such as finding the percentage by weight of elements in the compound.

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

Very pure hydrogen \((99.9 \%)\) can be made by which of the following proceses? (a) Reaction of methane with steam (b) Reaction of salt like hydrides with water (c) Electrolysis of water (d) Mixing natural hydrocarbons of high molecular weight

Sugarcane on reaction with nitric acid gives (a) \(2 \mathrm{HCOOH}\) (two moles) (b) \(\mathrm{CO}_{2}\) and \(\mathrm{SO}_{2}\) (c) no reaction (d) \((\mathrm{COOH})_{2}\)

\(\mathrm{H}_{2} \mathrm{O}_{2}\) exists as .... in alkaline medium. (a) \(\mathrm{HO}_{2}+\) (b) \(\mathrm{H}_{2} \mathrm{O}+\) (c) \(\mathrm{HO}_{2}-\) (d) \(\mathrm{O}_{2}^{2}-\)

A commercial sample of hydrogen peroxide is labelled as 10 volume, its percentage strength is (a) \(1 \%\) (b) \(3 \%\) (c) \(10 \%\) (d) \(90 \%\)

Nitrogen is a relatively inactive element because (a) dissociation energy of its molecule is fairly high (b) its electronegativity is fairly high (c) it has low atomic radius (d) its atom has a stable electronic configuration
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Kinetics

Read Explanation

Organic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Reactions

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.