Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 2: Problem 47

Explain an experiment to study the effect of temperature and concentration on the rate of reaction.

Short Answer

Expert verified
Answer: The key variables in this experiment are temperature and concentration. The steps involved in designing the experiment are: 1. Choose a suitable chemical reaction. 2. Gather materials and equipment. 3. Control other variables. 4. Prepare the reaction setup. 5. Perform the experiment at different temperatures. 6. Record the duration and volume of gas produced. 7. Analyze the data to determine the rate of reaction. 8. Draw conclusions about the effect of temperature and concentration on the rate of the reaction.

Step by step solution

01

Choose a suitable chemical reaction to study

Select a chemical reaction that is affected by both temperature and concentration, and has an observable change. One common example is the reaction between magnesium and hydrochloric acid, which produces hydrogen gas and has a noticeable rate of reaction. The reaction is: Mg(s) + 2HCl(aq) -> MgCl2(aq) + H2(g)
02

Gather materials and equipment

Make sure all necessary materials and equipment are available to conduct the experiment. These include: - Magnesium ribbon or powder - Hydrochloric acid (HCl) in different concentrations - A method to heat the solution (a water bath or electric heater) - Test tubes or flasks to perform the reaction in - Stopwatch to time the duration of the reaction - Measuring cylinder to measure the volume of gas produced (or a gas syringe)
03

Control variables

In order to ensure a fair experiment, all other variables except temperature and concentration must be controlled. Keep the size and shape of the magnesium samples consistent for each trial. Measure and mix the different concentrations of hydrochloric acid accurately.
04

Prepare the reaction setup

Set up the reaction vessels containing identical magnesium samples. Prepare the hydrochloric acid solutions with different concentrations (e.g. 0.5M, 1M, and 2M) and pour each one into separate reaction vessels.
05

Perform the experiment at different temperatures

Perform the reaction at various temperatures, like room temperature (25°C), moderately hot (40°C), and hot (50°C) using a water bath or electric heater to control the temperature. For each temperature setting, conduct the reaction with the hydrochloric acid at the chosen concentrations.
06

Record the duration and volume of gas produced

As soon as the reaction starts, use the stopwatch to time the duration of the reaction. Record the volume of hydrogen gas produced at different time intervals (e.g., every 10 seconds) using a measuring cylinder filled with water and inverted over the mouth of the reaction vessel or a gas syringe. Repeat the experiment for each concentration of hydrochloric acid at the different temperatures.
07

Analyze the data

Using the recorded data, determine the rate of reaction by calculating the volume of gas produced per unit of time for each trial. Compare the rates of reaction at different temperatures and concentrations to analyze the effect on the chemical reaction.
08

Draw conclusions

Based on the analysis, draw conclusions about the effect of temperature and concentration on the rate of the reaction. Discuss any patterns or trends observed and explain the findings using scientific principles, such as collision theory and the role of the activation energy in chemical reactions.

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 magnitude of decreases in the presence of a catalyst.

The reaction between \(\mathrm{Zn}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is an example for reaction.

When the reaction of synthesis of ammonia is carried out with a mixture of hydrogen and deuterium, what are the products obtained at the end of the process?

Product the shift in equilibrium when the volume is decreased on the following equilibrium reactions: (i) \(\mathrm{Pcl}_{3(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})} \rightleftarrows \mathrm{PCl}_{5(\mathrm{~g})}\) (ii) \(\mathrm{N}_{2(g)}+\mathrm{O}_{2(\mathrm{~g})} \rightleftarrows 2 \mathrm{NO}_{(g)}\)

State Le Chatlier's principle and apply it to the following equilibria: (i) \(2 \mathrm{NO}_{(\mathrm{g})} \rightleftarrows \mathrm{N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}+\) Heat (ii) \(\mathrm{N}_{2} \mathrm{O}_{4(\mathrm{~g})} \rightleftarrows 2 \mathrm{NO}_{2(\mathrm{~g})}-\) Heat
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Kinetics

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Making Measurements

Read Explanation

Organic Chemistry

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