A 1.000 g sample of naphthalene is burned in a 25.00 g aluminium calorimeter that contains 250.0 g of water. The temperature of the calorimeter and the water increases by 35.50°C. According to this data, the molar enthalpy of combustion of naphthalene is ♦ MJ/mol Record your 3-digit answer. Include sign; do not include units. Hint: Include both the water and the aluminium calorimeter in your calculation. Note that the units for your answer should be in MJ/mol. Use your recorded answer from Question 18 to answer the next question. That is, use the answer you recorded in the answer box, not your unrounded value. If the theoretical value for the molar enthalpy of combustion of naphthalene is - 5155.9 kJ/mol, then the percent error for this calorimetry experiment is %. Record your 3-digit answer; do not enter % sign. If 67.5 kJ of energy is transferred when 1.65 g of benzene is burned in a calorimeter, then the molar enthalpy of combustion of benzene expressed in scientific notation is +/-a.bc x10d kJ/mol. The values of a, b, c, and d are , and
A 1.000 g sample of naphthalene is burned in a 25.00 g aluminium calorimeter that contains 250.0 g of water. The temperature of the calorimeter and the water increases by 35.50°C. According to this data, the molar enthalpy of combustion of naphthalene is ♦ MJ/mol Record your 3-digit answer. Include sign; do not include units. Hint: Include both the water and the aluminium calorimeter in your calculation. Note that the units for your answer should be in MJ/mol. Use your recorded answer from Question 18 to answer the next question. That is, use the answer you recorded in the answer box, not your unrounded value. If the theoretical value for the molar enthalpy of combustion of naphthalene is - 5155.9 kJ/mol, then the percent error for this calorimetry experiment is %. Record your 3-digit answer; do not enter % sign. If 67.5 kJ of energy is transferred when 1.65 g of benzene is burned in a calorimeter, then the molar enthalpy of combustion of benzene expressed in scientific notation is +/-a.bc x10d kJ/mol. The values of a, b, c, and d are , and
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
Transcribed Image Text:Naphthalene (C₁0H8(s)) originally was used as the main ingredient in mothballs.
Its use was discontinued because of health concerns; exposure to large amounts
of naphthalene may damage or destroy red blood cells, cause confusion, nausea,
vomiting, diarrhea and jaundice. Naphthalene dust can be an explosion hazard
when exposed to heat or flame. It may ignite by friction, heat, sparks or flame. It
also may re-ignite after the fire is extinguished and containers of naphthalene
may explode when heated. The following calorimetry experiment was designed to
determine the enthalpy of combustion of naphthalene.
Fig. 1
Thermometer
Aluminium cover
Water
Aluminium calorimeter
A 1.000 g sample of naphthalene is burned in a 25.00 g aluminium calorimeter
that contains 250.0 g of water. The temperature of the calorimeter and the water
increases by 35.50°C. According to this data, the molar enthalpy of combustion
of naphthalene is
◆
hexamine tablet
MJ/mol
Record your 3-digit answer. Include sign; do not include units.
Hint: Include both the water and the aluminium calorimeter in your calculation.
Note that the units for your answer should be in MJ/mol.
Use your recorded answer from Question 18 to answer the next question. That is,
use the answer you recorded in the answer box, not your unrounded value.
%.
If the theoretical value for the molar enthalpy of combustion of naphthalene is -
5155.9 kJ/mol, then the percent error for this calorimetry experiment is
Record your 3-digit answer; do not enter % sign.
If 67.5 kJ of energy is transferred when 1.65 g of benzene is burned in a
calorimeter, then the molar enthalpy of combustion of benzene expressed in
scientific notation is +/-a.bc x10d kJ/mol. The values of a, b, c, and d are
◆
, and
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 4 steps with 6 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