Given the balanced chemical equation: Fe(s) +2 HCI(aq) FeCl2(aq) + H2(3) AHrxn ?? A sample of 0.93 g of Fe metal is combined with excess HCI to make 200 g of solution in a calorimeter and allowed to react completely. If the temperature of the solution rises from 25.0 °C to 29.6 °C, find AHrxn in kJ for this reaction. (Cs of soln = 4.184 J/g °C) (1 kJ=1000 J) Csoln, msoln AT 9soln 9rxn AHxn AHan = Arxn mol of Fe q=m xc x AT 9 rxn = -9soln %3D Include the sign for your value. Round and report your answer to an integer without decimal place.
Given the balanced chemical equation: Fe(s) +2 HCI(aq) FeCl2(aq) + H2(3) AHrxn ?? A sample of 0.93 g of Fe metal is combined with excess HCI to make 200 g of solution in a calorimeter and allowed to react completely. If the temperature of the solution rises from 25.0 °C to 29.6 °C, find AHrxn in kJ for this reaction. (Cs of soln = 4.184 J/g °C) (1 kJ=1000 J) Csoln, msoln AT 9soln 9rxn AHxn AHan = Arxn mol of Fe q=m xc x AT 9 rxn = -9soln %3D Include the sign for your value. Round and report your answer to an integer without decimal place.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Concept explainers
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
![**Determining Enthalpy Change (ΔH) for the Reaction of Fe with HCl**
Given the balanced chemical equation:
\[ \text{Fe}(s) + 2\, \text{HCl}(aq) \rightarrow \text{FeCl}_2(aq) + \text{H}_2(g) \]
\[ \Delta H_{\text{rxn}} \: \text{??} \]
A sample of 0.93 g of Fe metal is combined with excess HCl to make 200 g of solution in a calorimeter and allowed to react completely. If the temperature of the solution rises from 25.0 °C to 29.6 °C, find \(\Delta H_{\text{rxn}}\) in kJ for this reaction. \((C_s ~ \text{of solution} ~= ~4.184~J/g~°C)~(1~kJ = 1000~J)\)
**Analysis Steps:**
1. **Calculate the heat gained by the solution (\(q_{\text{soln}}\)):**
\[ q_{\text{soln}} = m_{\text{soln}} \times c_{\text{soln}} \times \Delta T \]
2. **Determine the heat of reaction (\(q_{\text{rxn}}\)):**
\[ q_{\text{rxn}} = - q_{\text{soln}} \]
3. **Calculate the enthalpy change (\(\Delta H_{\text{rxn}}\)) per mole of Fe:**
\[ \Delta H_{\text{rxn}} = \frac{q_{\text{rxn}}}{\text{mol of Fe}} \]
**Flow Diagram Explanation:**
The image provides a clear flow diagram to illustrate the step-by-step process used to determine \(\Delta H_{\text{rxn}}\):
1. **\(q_{\text{soln}}\):** The heat gained by the solution is calculated using the mass of the solution, the specific heat capacity of the solution, and the change in temperature.
2. **\(q_{\text{rxn}}\):** The heat of the reaction is the negative of the heat gained by the solution.
3. **\(\Delta H_{\text{rxn}}\):** The enthalpy change of the reaction is determined by dividing \(q_{\text{rxn}}\) by the number of moles](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5e5efc23-a198-4327-bdc7-d2931bd5f43b%2F4a30f893-dc2a-4010-ab1e-6b41a67838b2%2Fah2cysj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Determining Enthalpy Change (ΔH) for the Reaction of Fe with HCl**
Given the balanced chemical equation:
\[ \text{Fe}(s) + 2\, \text{HCl}(aq) \rightarrow \text{FeCl}_2(aq) + \text{H}_2(g) \]
\[ \Delta H_{\text{rxn}} \: \text{??} \]
A sample of 0.93 g of Fe metal is combined with excess HCl to make 200 g of solution in a calorimeter and allowed to react completely. If the temperature of the solution rises from 25.0 °C to 29.6 °C, find \(\Delta H_{\text{rxn}}\) in kJ for this reaction. \((C_s ~ \text{of solution} ~= ~4.184~J/g~°C)~(1~kJ = 1000~J)\)
**Analysis Steps:**
1. **Calculate the heat gained by the solution (\(q_{\text{soln}}\)):**
\[ q_{\text{soln}} = m_{\text{soln}} \times c_{\text{soln}} \times \Delta T \]
2. **Determine the heat of reaction (\(q_{\text{rxn}}\)):**
\[ q_{\text{rxn}} = - q_{\text{soln}} \]
3. **Calculate the enthalpy change (\(\Delta H_{\text{rxn}}\)) per mole of Fe:**
\[ \Delta H_{\text{rxn}} = \frac{q_{\text{rxn}}}{\text{mol of Fe}} \]
**Flow Diagram Explanation:**
The image provides a clear flow diagram to illustrate the step-by-step process used to determine \(\Delta H_{\text{rxn}}\):
1. **\(q_{\text{soln}}\):** The heat gained by the solution is calculated using the mass of the solution, the specific heat capacity of the solution, and the change in temperature.
2. **\(q_{\text{rxn}}\):** The heat of the reaction is the negative of the heat gained by the solution.
3. **\(\Delta H_{\text{rxn}}\):** The enthalpy change of the reaction is determined by dividing \(q_{\text{rxn}}\) by the number of moles
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 3 steps with 1 images
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
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY