Chemistry: An Introduction to General, Organic, and Biological Chemistry, Books a la Carte Edition & Modified MasteringChemistry with Pearson eText -- ValuePack Access Card Package
1st Edition
ISBN: 9780133899573
Author: Karen C. Timberlake
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 3, Problem 3.80AQAP
On a hot sunny day, you get out of the swimming pool and sit in a metal chair, which is very hot. Would you predict that the specific heat of the metal is higher or lower than that of water? Explain. (3.6)
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
When copper(II) sulfate pentahydrate (CuSO4·5 H2O) is heated, it decomposes to the dehydrated form. The waters of hydration are released from the solid crystal and form water vapor. The hydrated form is medium blue, and the dehydrated solid is light blue.
The balanced equation is CuSO4·5 H2O(s) --> CuSO4(s) + 5 H2O(g) *heat above the arrow
If 5.32 g CuSO4·5 H2O is decomposed to CuSO4, predict the mass of the remaining light blue solid.
an important flavor component of vanilla extract is vanillin C8H8O3 molar mass = 152.15 g/mol when vanillin burns in a bomb calorimeter with a heat capacity of 8.60 kJ/°C the temp increases from 25.97°C to 31.18°C. if the heat of combustion of vanillin is -3760 kJ/mol what mass of vanillin (in g) was combusted? answer to two decimal places
When 2 moles of H2S(g) react with O2(g) to form H2O(l) and SO2(g) according to the following equation, 1.12×103 kJ of energy are evolved.
2H2S(g) + 3O2(g)---->2H2O(l) + 2SO2(g)
Is this reaction endothermic or exothermic? _________(endothermic or exothermic)What is the value of q? ________kJ
Chapter 3 Solutions
Chemistry: An Introduction to General, Organic, and Biological Chemistry, Books a la Carte Edition & Modified MasteringChemistry with Pearson eText -- ValuePack Access Card Package
Ch. 3.1 - Classify each of the following as a pure substance...Ch. 3.1 - Classify each of the following as a pure substance...Ch. 3.1 - Prob. 3.3QAPCh. 3.1 - Prob. 3.4QAPCh. 3.1 - Prob. 3.5QAPCh. 3.1 - Prob. 3.6QAPCh. 3.2 - Prob. 3.7QAPCh. 3.2 - Indicate whether each of the following describes a...Ch. 3.2 - Describe each of the following as a physical or...Ch. 3.2 - Describe each of the following as a physical or...
Ch. 3.2 - Prob. 3.11QAPCh. 3.2 - What type of change, physical or chemical, takes...Ch. 3.2 - Describe each property of the element fluorine as...Ch. 3.2 - Describe each property of the element zirconium as...Ch. 3.3 - Prob. 3.15QAPCh. 3.3 - Prob. 3.16QAPCh. 3.3 - Prob. 3.17QAPCh. 3.3 - Calculate the unknown temperature in each of the...Ch. 3.3 - Prob. 3.19QAPCh. 3.3 - a. Water is heated to 145 °F. What is the...Ch. 3.4 - Discuss the changes in the potential and kinetic...Ch. 3.4 - Prob. 3.22QAPCh. 3.4 - Indicate whether each of the following statements...Ch. 3.4 - Prob. 3.24QAPCh. 3.4 - The energy needed to keep a 75-wattlight bulb...Ch. 3.4 - Prob. 3.26QAPCh. 3.5 - Calculate the kilocalories for each of the...Ch. 3.5 - Calculate the kilocalories for each of the...Ch. 3.5 - Using the energy values for foods (see TABLE3.7),...Ch. 3.5 - Using the energy values for foods (see TABLE3.7),...Ch. 3.5 - Prob. 3.31QAPCh. 3.5 - Prob. 3.32QAPCh. 3.6 - If the same amount of heat is supplied to samples...Ch. 3.6 - Substances A and B are the same mass and at the...Ch. 3.6 - Prob. 3.35QAPCh. 3.6 - Prob. 3.36QAPCh. 3.6 - Use the heat equation to calculate the energy, in...Ch. 3.6 - Use the heat equation to calculate the energy, in...Ch. 3.7 - Identify each of the following changes of state as...Ch. 3.7 - Identify each of the following changes of state as...Ch. 3.7 - Calculate the heat change at 0 °C for each of the...Ch. 3.7 - Prob. 3.42QAPCh. 3.7 - Identify each of the following changes of state as...Ch. 3.7 - Identify each of the following changes of state as...Ch. 3.7 - Prob. 3.45QAPCh. 3.7 - 3.50 Calculate the heat change at 100 °C for each...Ch. 3.7 - Prob. 3.47QAPCh. 3.7 - Prob. 3.49QAPCh. 3.7 - Prob. 3.50QAPCh. 3 - Prob. 3.51UTCCh. 3 - Prob. 3.52UTCCh. 3 - Prob. 3.53UTCCh. 3 - Prob. 3.54UTCCh. 3 - Prob. 3.55UTCCh. 3 - Prob. 3.56UTCCh. 3 - Prob. 3.57UTCCh. 3 - Prob. 3.58UTCCh. 3 - Calculate the energy to heat two cubes (gold and...Ch. 3 - Calculate the energy to heat two cubes (silver and...Ch. 3 - Prob. 3.61UTCCh. 3 - Prob. 3.62UTCCh. 3 - Prob. 3.63AQAPCh. 3 - Prob. 3.64AQAPCh. 3 - Prob. 3.65AQAPCh. 3 - Prob. 3.66AQAPCh. 3 - Prob. 3.67AQAPCh. 3 - Prob. 3.68AQAPCh. 3 - Prob. 3.69AQAPCh. 3 - Prob. 3.70AQAPCh. 3 - Prob. 3.71AQAPCh. 3 - Prob. 3.72AQAPCh. 3 - Prob. 3.73AQAPCh. 3 - Calculate each of the following temperatures in...Ch. 3 - What is 15 °F in degrees Celsius and in kelvins?...Ch. 3 - Prob. 3.76AQAPCh. 3 - Prob. 3.77AQAPCh. 3 - Prob. 3.78AQAPCh. 3 - Prob. 3.79AQAPCh. 3 - On a hot sunny day, you get out of the swimming...Ch. 3 - Prob. 3.81AQAPCh. 3 - Prob. 3.82AQAPCh. 3 - A 0.50-g sample of vegetable oil is placed in a...Ch. 3 - A 1.3-g sample of rice is placed in a calorimeter....Ch. 3 - Prob. 3.85AQAPCh. 3 - Prob. 3.86AQAPCh. 3 - The melting point of dibromomethane is 53 °C and...Ch. 3 - Prob. 3.88AQAPCh. 3 - Prob. 3.89CQCh. 3 - A 45-g piece of ice at 0.0 °C is added to a sample...Ch. 3 - Prob. 3.91CQCh. 3 - Prob. 3.92CQCh. 3 - Prob. 3.93CQCh. 3 - A 115-g sample of steam at 100 °C is emitted from...Ch. 3 - Prob. 1CICh. 3 - Prob. 2CICh. 3 - Answer the following for water samples A and B...Ch. 3 - Prob. 4CICh. 3 - Prob. 5CICh. 3 - Prob. 6CI
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
- 9.85 The figure below shows a "self-cooling" beverage can. The can is equipped with an outer jacket containing sodium carbonate (Na2CO3), which dissolves in water rapidly and endothermically: Na2CO3(s)2Na+(aq)+CO32(aq) H= 67.7 kJ The user adds water to the outer jacket, and the heat absorbed in the chemical reaction chills the drink. The can contains 200 g of drink, the jacket contains 55 g of Na2CO3, and 100 g of water is to be added. If the initial temperatures of the can and the water are both 32°C on a summer day, what is the coldest temperature that the drink can reach? The can itself has a heat capacity of 40 J/C Assume that the Na2CO3 solution and the drink both have the same heat capacity as pure water, 4.184 J g-l C-l, (HINT: Treat this like a calorimetry problem.)arrow_forwardA calorimeter is charged with 57.9 mL of water at 25.0 °C. After a reaction takes place in the calorimeter, the water temperature is 26.4 °C. How much heat did the reaction produce, and was it exothermic or endothermic? (The density of water is 1.00 g/mL.)arrow_forwardYou have a piece of iron, the specific heat of iron, the specific heat of iron is 0.449 J/g °C and the change in temperature is 5.7°C. If you add 307 J to the iron. what its mass?arrow_forward
- A piece of parmesan cheese is burned in a soda can calorimeter, and heats up 0.235 kg of water by 2.85 °C. The calorimeter was calibrated and had a calorimetry constant of 8.50 kcal/kg･°C. Given that protein contains 4.00 kcal/g, calculate the mass in g of the protein contained in the parmesan. Assume that the cheese is composed primarily of protein.arrow_forwardWhat is the specific heat of a 53.01 g piece of an unknown metal that exhibits a 45.2°C temperature change upon absorbing 1870 J of heat? (Answer in J/g*°C)arrow_forwardDuncan takes a break from studying and goes to the gym to swim laps. If swimming burns 9.05×105 calcal per hour, how many kilojoules does swimming burn in that same amount of time? In other words, convert 9.05×105 calcal to kilojoules.arrow_forward
- A) A hamburger comtains 409 kilocalories(409 cal). How many kJ is this? B) If a jogger burns 1225 kJ during her 5-mile run, How many kilocalories did she use up? How many hamburgers will it take to replace those kilojoules that she used up?arrow_forward1. How many KJ are used by a 154lb adult while sleeping for one hour? 2. In the specific heat equation the delta T symbol (?T) stands for?arrow_forwardEthylene (C2H4) is the starting material for the preparation of polyethylene. It is usually made during the manufacturing of petroleum. It occurs as a fruit-ripening hormone and a component of natural gas. If the heat of combustion of C2H4 is -1411 kJ/mg. how many grams of the ethylene must be burned to give 70.0 kJ of heat? a. 3.29 grams b. 1.39 grams c. 9.21 grams d. 2.19 gramsarrow_forward
- A 27 g aluminum foil pan is used to roast vegetables. The pan is put into a cold oven at 22 oC . How much energy in cal is absorbed by the pan after cooking at 232 oC (450. oF) for 25 minutes?arrow_forwardQuestion: Silver Nitrate and hydrochloric acid combine to make 100.0 mL of aqueous solution in a coffee cup calorimeter. The temperature changes from 23.40 degrees C to 24.21 degrees C. - Calculate the heat released by the reaction (find qrxn) - If 50.0 mL of a 0.100 M AgNO3 reacts completely, calculate the moles of AgNO3 that reacted. - Using your answers for parts a and b, calculate triangleHrxn for this reaction in units of kJ/mol.arrow_forwardConsider the following balanced thermochemical equationfor a reaction sometimes used for H₂S production:1/8S₈(s)+H2(g)→H₂S Hᵣₓₙ=-20.2kJ(a) Is this an exothermic or endothermic reaction?(b) What is ΔHᵣₓₙ for the reverse reaction?(c) What is ΔH when 2.6 mol of S₈ reacts?(d) What is ΔH when 25.0 g of S₈ reacts?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY