Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 14: Problem 14

For each of these pairs of reaction conditions, indicate which has the faster rate of formation of hydrogen gas: (a) sodium or potassium with water, (b) magnesium or iron with \(1.0 \mathrm{M} \mathrm{HCl}\), (c) magnesium rod or magnesium powder with \(1.0 \mathrm{M} \mathrm{HCl}\), (d) magnesium with \(0.10 M \mathrm{HCl}\) or magnesium with \(1.0 \mathrm{M} \mathrm{HCl}\).

Short Answer

Expert verified
The conditions with the faster rate of formation of hydrogen gas would be (a) potassium with water, (b) magnesium with \(1.0 \mathrm {M} \mathrm {HCl}\), (c) magnesium powder with \(1.0 \mathrm {M} \mathrm {HCl}\), and (d) magnesium with \(1.0 \mathrm {M} \mathrm {HCl}\).

Step by step solution

01

Reactivity of Elements

In the reactivity series, potassium is more reactive than sodium, magnesium is more reactive than iron, and all are more reactive than hydrogen. Therefore, potassium will react more quickly than sodium with water, and magnesium will react more quickly than iron with \(1.0 \mathrm {M} \mathrm{HCl}\).
02

Role of Surface Area

The rate of a reaction increases with an increase in surface area, because more surface area means more space for collisions to occur between reacting particles. Therefore, magnesium powder will react more quickly than a magnesium rod with \(1.0 \mathrm {M} \mathrm {HCl}\), as the powder has a greater surface area compared to the rod.
03

Role of Concentration

The rate of a reaction increases with an increase in concentration of the reactants, because a higher concentration means more particles in the same volume, leading to more collisions. Therefore, magnesium is expected to react more quickly with \(1.0 \mathrm {M} \mathrm {HCl}\) than with \(0.1 \mathrm {M} \mathrm {HCl}\).

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

On which of these quantities does the rate constant of a reaction depend: (a) concentrations of reactants, (b) nature of reactants, (c) temperature?

What are the characteristics of a catalyst?

“The rate constant for the reaction $$ \mathrm{NO}_{2}(g)+\mathrm{CO}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{CO}_{2}(g) $$ is \(1.64 \times 10^{-6} / M \cdot \mathrm{s} .\)." What is incomplete about this statement?

When a mixture of methane and bromine is exposed to light, the following reaction occurs slowly: $$ \mathrm{CH}_{4}(g)+\mathrm{Br}_{2}(g) \longrightarrow \mathrm{CH}_{3} \mathrm{Br}(g)+\mathrm{HBr}(g) $$ Suggest a reasonable mechanism for this reaction. (Hint: Bromine vapor is deep red; methane is colorless.)

As we know, methane burns readily in oxygen in a highly exothermic reaction. Yet a mixture of methane and oxygen gas can be kept indefinitely without any apparent change. Explain.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Inorganic Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Analysis

Read Explanation

Nuclear Chemistry

Read Explanation

Making Measurements

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