Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
The energy content of food is typically determined using a bomb calorimeter. Consider the combustion of a 0.30-g sample of butter in a bomb calorimeter having a heat capacity of 2.67 kJ/°C. If the temperature of the calorimeter increases from 23.5°C to 26.9°C, calculate the energy of combustion per gram of butter.
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 nowThis is a popular solution!
Step by stepSolved in 5 steps
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.Similar questions
- A student conducts a calorimetry experiment on an unknown metal object. The unknown metal object with a mass of 82.522 g is heated to 100.5 °C and then transferred to a coffee-cup calorimeter containing 67.225 g of water at 22.3 °C. If the metal object and the water reach a final temperature of 30.5 °C and the heat absorbed by the water was calculated to be 2310 J. What is the specific heat of this metal object? (The specific heat of water is 4.18 J/g°C)arrow_forwardAcetylene, c2h2, is used in welding torches. It releases a lot of energy when burned in oxygen. The combustion of one gram of acetylene releases 48.2 kJ. A 0.750-gram sample of acetylene is burned in a bomb calorimeter (heat capacity = 1.117kJ/C) that contains 800.0 g of water. The final temperature of the bomb and water after combustion is 35.2C. What is the initial temperature of the bomb and water?arrow_forwardIn a coffee-cup calorimeter, 130.0 mL of 1.0 M NaOH and 130.0 mL of 1.0 M HCI are mixed. Both solutions were originally at 21.7°C. After the reaction, the final temperature is 28.4°C. Assuming that all the solutions have a density of 1.0 g/cm3 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCl by NAOH . Assume that no heat is lost to the surroundings or to the calorimeter. DeltaH = ____________kJ/molarrow_forward
- A piece of chromium metal with a mass of 24.64 g is heated in boiling water to 98.3 °C and then dropped into a coffee-cup calorimeter containing 82.3 g of water at 22.6 °C. When thermal equilibrium is reached, the final temperature is 25.0 °C. Calculate the specific heat capacity of chromium. (The specific heat capacity of liquid water is 4.184 J/g ⋅ K.)arrow_forwardYou can find the amount of heat evolved in the combustion of carbon by carrying out the reaction in a combustion calorimeter. You burn 0.300 g of carbon (graphite) in an excess of O2(g) to give CO2(g). C (graphite) + O2(g) → CO2(g) The temperature of the calorimeter, which contains 775 g of water, increases from 25.0˚C to 27.38˚C. What quantity of heat is evolved per mole of carbon?arrow_forwardIn a coffee-cup calorimeter, 110.0 mL of 1.1 M NaOH and 110.0 mL of 1.1 M HCl are mixed. Both solutions were originally at 22.1°C. After the reaction, the final temperature is 29.5°C. Assuming that all the solutions have a density of 1.0 g/ cm° and a specific heat capacity of 4.18 J/°C•g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. ΔΗ= kJ/molarrow_forward
- how to approacharrow_forwardA coffee-cup calorimeter is filled with 150.0 mL of water at 22.1 °C. A piece of metal at 121.4 °C with a mass of 16.5 g is added. The final temperature of the water and metal in the calorimeter is 24.5 °C. The density of liquid water is 1.00 g/mL, and its specific heat capacity is 4.18 J/(g·°C). Determine the specific heat capacity of the metal. a) 1.40 J/g∙oC b) 0.40 J/g∙oC c) 4.18 J/g∙oC d) 0.94 J/g∙oCarrow_forward1 Cal= 4.18 kJarrow_forward
- A 93.82 g bar of iron was heated to 98.4 °C and then dropped into 38.1 mL of water at 15.3 °C. The temperature of the water increased to a maximum of 32.7 °C. Calculate the specific heat capacity of iron. Assume that the density of water is 1.00 g/mL. heat capacity (J/g°C)arrow_forward150. g of water (Cs = 4.184 J/g°C) at 20.0 °C is added to a coffee cup calorimeter. A 35.0 g sample of silver (Cs = 0.129 J/g°C) is then placed into the water. At thermal equilibrium, the temperature of the calorimeter is 22.07 °C. What was the initial temperature of the silver sample?arrow_forward15.0 mL of a strong base is added to 15.0 mL of a strong acid in a coffee cup calorimeter. The temperature of the calorimeter contents rises from 22.5 °C to 24.5 °C. Assume that: concentration of base = 0.500 M concentration of acid = 0.500 M the specific heat of the solution is 4.184 J/g°C the density of the solution is 1.00 g/mL the coffee cup does not absorb or release energy itself Calculate the ΔH for this neutralization reaction in kJ per mole of base. Group of answer choices –0.299 kJ/mol –0.502 kJ/mol –16.7 kJ/mol –33.5 kJ/molarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
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