Homework Help is Here – Start Your Trial Now!
Science
Chemistry
A student dissolves 13.8 g of ammonium chloride (NH4Cl) in 250. g of water in a well-insulated open cup. She then observes the temperature of the water from 21.0 °C to 17.3 °C over the course of 6.3 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH₂Cl(s) - - • NH (aq) + C1 (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known an published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy AHxn per mole of NH4Cl. exothermic O endothermic O neither ☐ kJ 0 kJ mol X

A student dissolves 13.8 g of ammonium chloride (NH4Cl) in 250. g of water in a well-insulated open cup. She then observes the temperature of the water from 21.0 °C to 17.3 °C over the course of 6.3 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH₂Cl(s) - - • NH (aq) + C1 (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known an published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy AHxn per mole of NH4Cl. exothermic O endothermic O neither ☐ kJ 0 kJ mol X

Chemistry
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...
See similar textbooks
icon
Related questions
Question
A student dissolves 13.8 g of ammonium chloride (NH4Cl) in 250. g of water in a well-insulated open cup. She then observes the temperature of the water from 21.0 °C to 17.3 °C over the course of 6.3 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH₂Cl(s) → NH(aq) + Cl¯ (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to t correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy AH per mole of NH Cl. exothermic O endothermic Oneither 0 kJ 1 kJ mol x10 Ś
Transcribed Image Text:A student dissolves 13.8 g of ammonium chloride (NH4Cl) in 250. g of water in a well-insulated open cup. She then observes the temperature of the water from 21.0 °C to 17.3 °C over the course of 6.3 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH₂Cl(s) → NH(aq) + Cl¯ (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to t correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy AH per mole of NH Cl. exothermic O endothermic Oneither 0 kJ 1 kJ mol x10 Ś
Expert Solution
Step 1

a.) Nature of reaction can be determined from temperature change. 

b.) Heat can be calculated using formula

Q = mC∆T 

c.) ∆H is Calculate using formula

∆H = Q / n 

steps

Step by step

Solved in 3 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Thermodynamics
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.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS