Homework Help is Here – Start Your Trial Now!
Engineering
Chemical Engineering
When 2.76 g of potassium carbonate was added to 30.0 cm³ of approximately 2 mol dm-3 hydrochloric acid, the temperature rose by 5.20 °C. (i) Write an equation, including state symbols, for this reaction. (ii) Calculate the enthalpy change for this reaction per mole of potassium carbonate. Assume that the specific heat capacity and density of all solutions are 4.18 J g-1K-1 and 1.00 g cm-3 respectively. (iii) Explain why the hydrochloric acid need only be approximately 2 mol dm-3.

When 2.76 g of potassium carbonate was added to 30.0 cm³ of approximately 2 mol dm-3 hydrochloric acid, the temperature rose by 5.20 °C. (i) Write an equation, including state symbols, for this reaction. (ii) Calculate the enthalpy change for this reaction per mole of potassium carbonate. Assume that the specific heat capacity and density of all solutions are 4.18 J g-1K-1 and 1.00 g cm-3 respectively. (iii) Explain why the hydrochloric acid need only be approximately 2 mol dm-3.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
See similar textbooks
icon
Related questions
Question
Full solution pls
a) When 2.76 g of potassium carbonate was added to 30.0 cm³ of approximately 2 mol dm-3 hydrochloric acid, the temperature rose by 5.20 °C. (i) Write an equation, including state symbols, for this reaction. (ii) Calculate the enthalpy change for this reaction per mole of potassium carbonate. Assume that the specific heat capacity and density of all solutions are 4.18 J g-1K-1 and 1.00 g cm3 respectively. (iii) Explain why the hydrochloric acid need only be approximately 2 mol dm-3. b) When 2.00 g of potassium hydrogencarbonate was added to 30.0 cm3 of the same hydrochloric acid, the temperature fell by 3.70 °C. (i) Write an equation, including state symbols, for this reaction. (ii) Calculate the enthalpy change for this reaction per mole of potassium hydrogencarbonate. c) When potassium hydrogencarbonate is heated, it decomposes into potassium carbonate, carbon dioxide and water. By applying Hess' Law and your results in (a) and (b), calculate the enthalpy change for the decomposition of potassium hydrogencarbonate.
Transcribed Image Text:a) When 2.76 g of potassium carbonate was added to 30.0 cm³ of approximately 2 mol dm-3 hydrochloric acid, the temperature rose by 5.20 °C. (i) Write an equation, including state symbols, for this reaction. (ii) Calculate the enthalpy change for this reaction per mole of potassium carbonate. Assume that the specific heat capacity and density of all solutions are 4.18 J g-1K-1 and 1.00 g cm3 respectively. (iii) Explain why the hydrochloric acid need only be approximately 2 mol dm-3. b) When 2.00 g of potassium hydrogencarbonate was added to 30.0 cm3 of the same hydrochloric acid, the temperature fell by 3.70 °C. (i) Write an equation, including state symbols, for this reaction. (ii) Calculate the enthalpy change for this reaction per mole of potassium hydrogencarbonate. c) When potassium hydrogencarbonate is heated, it decomposes into potassium carbonate, carbon dioxide and water. By applying Hess' Law and your results in (a) and (b), calculate the enthalpy change for the decomposition of potassium hydrogencarbonate.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Optimization process
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemical-engineering and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Introduction to Chemical Engineering Thermodynami…
Introduction to Chemical Engineering Thermodynami…
Chemical Engineering
ISBN:
9781259696527
Author:
J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:
McGraw-Hill Education
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemical Engineering
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
Elements of Chemical Reaction Engineering (5th Ed…
Elements of Chemical Reaction Engineering (5th Ed…
Chemical Engineering
ISBN:
9780133887518
Author:
H. Scott Fogler
Publisher:
Prentice Hall
Process Dynamics and Control, 4e
Process Dynamics and Control, 4e
Chemical Engineering
ISBN:
9781119285915
Author:
Seborg
Publisher:
WILEY
Industrial Plastics: Theory and Applications
Industrial Plastics: Theory and Applications
Chemical Engineering
ISBN:
9781285061238
Author:
Lokensgard, Erik
Publisher:
Delmar Cengage Learning
Unit Operations of Chemical Engineering
Unit Operations of Chemical Engineering
Chemical Engineering
ISBN:
9780072848236
Author:
Warren McCabe, Julian C. Smith, Peter Harriott
Publisher:
McGraw-Hill Companies, The
SEE MORE TEXTBOOKS