Chapter 7 Rate of chemical reactions Section 7.1 Investigating the rate of chemical reactions Experiment 7.1.1 Measuring the rate of reaction Purpose To measure the rate of reaction and investigate the effect of particle size and concentration on the rate. Theory Marble chips are composed of the ionic compound calcium carbonate. When chips are added to a hydrochloric acid solution the reaction that occurs produces carbon dioxide gas. Provided that no liquid 'spray' is able to leave the flask in which the reaction occurs, only carbon dioxide gas will be lost from the flask as the reaction proceeds. The equation for the reaction is: 2HCI(aq) + CaCo,(s) → CaCl,(aq) + H,0(1) + CO,(g) The mass loss is equal to the mass of carbon dioxide evolved. Duration 40 minutes Materials 40 ml 2.0 M hydrochloric acid (HCI) 20 ml 1.0 M hydrochloric acid (HCI) 40 g large marble chips 20 g small marble chips (do not use powdered chips) 3x 100 ml conical flasks 100 mL measuring cylinder 50 mL beaker cotton wool electronic balance computer and spreadsheet program (optional) Safety Wear safety glasses and a laboratory coat for this experiment. Hydrochloric acid solutions are corrosive and are an irritant to eyes, skin and respiratory system. Procedure Part A-Measuring reaction rate Using a measuring cylinder, pour 20 ml 2.0 M HCI into a 50 mL beaker. 2 Weigh approximately 20 g large marble chips into a 100 mL conical flask and loosely place a cotton wool plug in the neck of the flask. 3 Place the conical flask and the beaker of acid on the balance pan and tare the balance so that it reads zero. Carefully and quickly remove the cotton wool plug, add the acid to the flask, replace the beaker on the balance pan beside the flask, and replace the plug. Immediately start a stop-watch. 1 Copyright O Pearson Australia 2016 (a division of Pearson Australla Group Pty Ltd) ISBN 978 1 4886 1125 4 Page 1 Note the reading on the balance after 15 seconds, 30 seconds and at 30 second intervals thereafter. Continue for up to 10 minutes. 5 Draw up a table to record the mass loss (from the total starting mass) and the time, in minutes, from the start of the reaction. This could be done using a spreadsheet or graphing package. 6 Plot a graph of the mass loss against time. 4. tttn Part C-Effect of concentration Repeat the experiment as described in Part A, but this time use 20 mL 1.0 M HCI. Plot the graph of this data on the same set of axes as the first experiment.
Chapter 7 Rate of chemical reactions Section 7.1 Investigating the rate of chemical reactions Experiment 7.1.1 Measuring the rate of reaction Purpose To measure the rate of reaction and investigate the effect of particle size and concentration on the rate. Theory Marble chips are composed of the ionic compound calcium carbonate. When chips are added to a hydrochloric acid solution the reaction that occurs produces carbon dioxide gas. Provided that no liquid 'spray' is able to leave the flask in which the reaction occurs, only carbon dioxide gas will be lost from the flask as the reaction proceeds. The equation for the reaction is: 2HCI(aq) + CaCo,(s) → CaCl,(aq) + H,0(1) + CO,(g) The mass loss is equal to the mass of carbon dioxide evolved. Duration 40 minutes Materials 40 ml 2.0 M hydrochloric acid (HCI) 20 ml 1.0 M hydrochloric acid (HCI) 40 g large marble chips 20 g small marble chips (do not use powdered chips) 3x 100 ml conical flasks 100 mL measuring cylinder 50 mL beaker cotton wool electronic balance computer and spreadsheet program (optional) Safety Wear safety glasses and a laboratory coat for this experiment. Hydrochloric acid solutions are corrosive and are an irritant to eyes, skin and respiratory system. Procedure Part A-Measuring reaction rate Using a measuring cylinder, pour 20 ml 2.0 M HCI into a 50 mL beaker. 2 Weigh approximately 20 g large marble chips into a 100 mL conical flask and loosely place a cotton wool plug in the neck of the flask. 3 Place the conical flask and the beaker of acid on the balance pan and tare the balance so that it reads zero. Carefully and quickly remove the cotton wool plug, add the acid to the flask, replace the beaker on the balance pan beside the flask, and replace the plug. Immediately start a stop-watch. 1 Copyright O Pearson Australia 2016 (a division of Pearson Australla Group Pty Ltd) ISBN 978 1 4886 1125 4 Page 1 Note the reading on the balance after 15 seconds, 30 seconds and at 30 second intervals thereafter. Continue for up to 10 minutes. 5 Draw up a table to record the mass loss (from the total starting mass) and the time, in minutes, from the start of the reaction. This could be done using a spreadsheet or graphing package. 6 Plot a graph of the mass loss against time. 4. tttn Part C-Effect of concentration Repeat the experiment as described in Part A, but this time use 20 mL 1.0 M HCI. Plot the graph of this data on the same set of axes as the first experiment.
Chapter12: Chemical Kinetics
Section: Chapter Questions
Problem 9RQ
Related questions
Question
What are limitations and improvements in this experiment and source of errors
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:
9781285869759
Author:
Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:
Cengage Learning