Zinc metal reacts with HCl according to the following balanced equation: Zn(s) + 2HCl(aq) --> ZnCl2(aq) + H2(g) When 0.130 grams of Zn(s) is combined with an excess amount of HCl to make 48.0 mL of solution in a coffee-cup calorimeter, all the zinc reacts, raising the temperature of the solution from 21.70ºC to 24.00ºC. Find ΔH for this reaction in kJ/mol. Assume the density of the solution is 1.01 g/mL and the specific heat capacity of the solution is 4.184 J/gºC. Use an atomic weight of 65.38 g/mol for Zn
Zinc metal reacts with HCl according to the following balanced equation: Zn(s) + 2HCl(aq) --> ZnCl2(aq) + H2(g) When 0.130 grams of Zn(s) is combined with an excess amount of HCl to make 48.0 mL of solution in a coffee-cup calorimeter, all the zinc reacts, raising the temperature of the solution from 21.70ºC to 24.00ºC. Find ΔH for this reaction in kJ/mol. Assume the density of the solution is 1.01 g/mL and the specific heat capacity of the solution is 4.184 J/gºC. Use an atomic weight of 65.38 g/mol for Zn
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.62QE: A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup...
Related questions
Question
Question 13 (Ch.7)
Zinc metal reacts with HCl according to the following balanced equation:
Zn(s) + 2HCl(aq) --> ZnCl2(aq) + H2(g)
When 0.130 grams of Zn(s) is combined with an excess amount of HCl to make 48.0 mL of solution in a coffee-cup calorimeter, all the zinc reacts, raising the temperature of the solution from 21.70ºC to 24.00ºC. Find ΔH for this reaction in kJ/mol.
Assume the density of the solution is 1.01 g/mL and the specific heat capacity of the solution is 4.184 J/gºC.
Use an atomic weight of 65.38 g/mol for Zn
Hints:
-q(reaction) = q(solution)
ΔH = q/mol of limiting reagent
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 with 2 images
Recommended textbooks for you
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
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