Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 5, Problem 40QAP
Acetone peroxide, C9H18O6(s), is a powerful but highly unstable explosive that does not contain nitrogen. It can pass undetected through scanners designed to detect the presence of nitrogen in explosives like TNT (trinitrotoluene, C7H5N3O6), or ammonium nitrate.
(a) Write a balanced equation for the combustion (burning in oxygen) of acetone peroxide producing steam and carbon dioxide.
(b) What pressure is generated in a 2.00-L bottle when 5.00 g of acetone peroxide is ignited to 555°C and burned in air? Assume 100% combustion.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
What is the specific heat of gaseous Xe at constant volume (give answer in J/(kg*K)).
Calculate the amount of energy released as heat by the formation of 1.00 mL of water from a stoichiometric mixture of H2(g) and O2(g) at 25°C and a constant pressure of one bar. Calculate the amount of energy released as heat by this reaction per mole and per gram of H2(g). Take the density of water to be 1.00 grams per milliliter.
While the majority component of air is nitrogen (N2 ), the gas is very unreactive because of its stability due to the triplebonds that hold the nitrogen atoms together. Nitrogen gas is, therefore, relatively unavailable for chemical reactions.One of the few ways to “fix” nitrogen, making a nitrogen compound from the elemental nitrogen in the atmosphere, isthe Haber process (aka Haber-Bosch process). In this reaction, nitrogen gas combines with hydrogen gas to yieldammonia. The enthalpy (ΔH) of this reaction is −92.22 kJ.This process was discovered by the German chemist Fritz Haber in the early twentieth century. Through extensiveexperimentation, Haber found the conditions that would produce adequate yields (at a temperature of about 500 o C anda pressure of about 200 atm). This process holds a significant importance today because of its application in theindustrial production of ammonia-based fertilizer. In 1918, Haber received the Nobel Prize in Chemistry for his work.However, a lot…
Chapter 5 Solutions
Chemistry: Principles and Reactions
Ch. 5 - Prob. 1QAPCh. 5 - A 6.00-ft cylinder has a radius of 26 in. It...Ch. 5 - Prob. 3QAPCh. 5 - Prob. 4QAPCh. 5 - A cylinder with a movable piston records a volume...Ch. 5 - A tank is filled with gas to a pressure of 875 mm...Ch. 5 - A sample of CO2 gas at 22C and 1.00 atm has a...Ch. 5 - A sample of nitrogen gas has a pressure of 1.22...Ch. 5 - Prob. 9QAPCh. 5 - A tire is inflated to a gauge pressure of 28.0 psi...
Ch. 5 - Prob. 11QAPCh. 5 - A sealed tank at room temperature, 25C, has 22.0 g...Ch. 5 - A balloon filled with helium hasa volume of...Ch. 5 - Prob. 14QAPCh. 5 - Prob. 15QAPCh. 5 - Prob. 16QAPCh. 5 - A piece of dry ice (CO2(s)) has a mass of 22.50 g....Ch. 5 - A four-liter tank is filled with propane gas,...Ch. 5 - Prob. 19QAPCh. 5 - Prob. 20QAPCh. 5 - Calculate the densities (in g/L) of the following...Ch. 5 - Calculate the densities (in grams per liter) of...Ch. 5 - Helium-filled balloons rise in the air because the...Ch. 5 - Space probes to Mars have shown that its...Ch. 5 - Cyclopropane mixed in the proper ratio with oxygen...Ch. 5 - Phosgene is a highly toxic gas made up of carbon,...Ch. 5 - The gas in the discharge cell of a laser contains...Ch. 5 - Exhaled air contains 74.5% N2, 15.7% O2, 3.6% CO2,...Ch. 5 - A 1.58-g sample of C2H3X3(g) has a volume of 297...Ch. 5 - A 0.750-g sample of the gas PX3 is in a sealed...Ch. 5 - Nitrogen oxide is a pollutant commonly found in...Ch. 5 - Nitrogen trifluoride gas reacts with steam to...Ch. 5 - Dichlorine oxide is used as bactericide to purify...Ch. 5 - Titanium(III) chloride is used in the manufacture...Ch. 5 - Nitric acid can be prepared by bubbling dinitrogen...Ch. 5 - Potassium peroxide is used to absorb the CO2...Ch. 5 - Hydrogen cyanide (HCN) is a poisonous gas. It can...Ch. 5 - When hydrogen peroxide decomposes, oxygen is...Ch. 5 - Ammonium nitrate can be used as an effective...Ch. 5 - Acetone peroxide, C9H18O6(s), is a powerful but...Ch. 5 - Prob. 41QAPCh. 5 - A certain laser uses a gas mixture consisting of...Ch. 5 - A sample of a smoke stack emission was collected...Ch. 5 - Prob. 44QAPCh. 5 - Prob. 45QAPCh. 5 - Prob. 46QAPCh. 5 - Prob. 47QAPCh. 5 - Follow the instructions of Problem 47 for the...Ch. 5 - When acetylene, C2H2, is burned in oxygen, carbon...Ch. 5 - When ammonium nitrate decomposes at 722C,...Ch. 5 - Prob. 51QAPCh. 5 - Nitrogen gas can be obtained by decomposing...Ch. 5 - Prob. 53QAPCh. 5 - Prob. 54QAPCh. 5 - Prob. 55QAPCh. 5 - Prob. 56QAPCh. 5 - A gas effuses 1.55 times faster than propane...Ch. 5 - A gas effuses through an opening one-fifth as fast...Ch. 5 - Prob. 59QAPCh. 5 - Prob. 60QAPCh. 5 - At what temperature will a molecule of uranium...Ch. 5 - Calculate the average speed of a (a) chlorine...Ch. 5 - Prob. 63QAPCh. 5 - Prob. 64QAPCh. 5 - Prob. 65QAPCh. 5 - Prob. 66QAPCh. 5 - Prob. 67QAPCh. 5 - Prob. 68QAPCh. 5 - Prob. 69QAPCh. 5 - Given that 1.00 mol of neon and 1.00 mol of...Ch. 5 - An intermediate reaction used in the production of...Ch. 5 - Prob. 72QAPCh. 5 - Prob. 73QAPCh. 5 - Glycine is an amino acid made up of carbon,...Ch. 5 - Prob. 75QAPCh. 5 - The Lamborghini Aventador engine has a 12-cylinder...Ch. 5 - Prob. 77QAPCh. 5 - Prob. 78QAPCh. 5 - Prob. 79QAPCh. 5 - Prob. 80QAPCh. 5 - Prob. 81QAPCh. 5 - Prob. 82QAPCh. 5 - Prob. 83QAPCh. 5 - The graph below shows the distribution of...Ch. 5 - Consider the following sketch. Each square in bulb...Ch. 5 - The following figure shows three 1.00-L bulbs...Ch. 5 - Prob. 87QAPCh. 5 - Prob. 88QAPCh. 5 - Prob. 89QAPCh. 5 - Prob. 90QAPCh. 5 - Prob. 91QAPCh. 5 - A 0.2500-g sample of an Al-Zn alloy reacts with...Ch. 5 - Prob. 93QAPCh. 5 - A mixture in which the mole ratio of hydrogen to...
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
- Suppose that 1.00 kJ of heat is transferred to 2.00 mol argon(at 298 K, 1 atm). What will the final temperature Tf be if theheat is transferred (a) at constant volume, or (b) at constantpressure? Calculate the energy change, DU, in each case.arrow_forwardHow many liters of CO2 can be generated from fermentation process involving 200.5 g C6H12O6? The process has been done in a room with a temperature of 28°C and a pressure of 1.02 atmarrow_forwardNatural gas is very abundant in many Middle Eastern oilfields. However, the costs of shipping the gas to markets inother parts of the world are high because it is necessary toliquefy the gas, which is mainly methane and has a boilingpoint at atmospheric pressure of -164 °C. One possiblestrategy is to oxidize the methane to methanol, CH3OH,which has a boiling point of 65 °C and can therefore beshipped more readily. Suppose that 10.7 * 109 ft3 of methaneat atmospheric pressure and 25 °C is oxidized to methanol.(a) What volume of methanol is formed if the densityof CH3OH is 0.791 g>mL? (b) Write balanced chemicalequations for the oxidations of methane and methanol toCO21g2 and H2O1l2. Calculate the total enthalpy changefor complete combustion of the 10.7 * 109 ft3 of methanejust described and for complete combustion of the equivalentamount of methanol, as calculated in part (a).(c) Methane, when liquefied, has a density of 0.466 g>mL;the density of methanol at 25 °C is 0.791…arrow_forward
- 4a Assume that worldwide combustion of fossil fuel accounts for an energy use of 500 x 1015 kJ/year. Also, assume that all fossil fuels can be represented by the formula C3H5 with energy content of 32,500 kJ/kg.Finally, assume that air is 79% N2 and 21% O2 , and has a molecular weight of 29 kg/kmol. i. Estimate the annual release of CO2 to the atmosphere by burning fossil fuels, in kg/yr ii. If all that CO2 entered the atmosphere (and none was removed), estimate the increase in atmospheric concentration, in ppm by volume. Assume the atmosphere contains 6.7 x 1018 kg of air.arrow_forwardAt 273 K and 1 atm pressure, 1 mol of an ideal gas occupies 22.4 LIn which parts of the atmosphere would you expect gases to behave most ideally (ignoring any photochemical reactions)?arrow_forward13.3p. If you allow one pound of carbon dioxide to sublime (change from CO2(s) to CO2(g)) at room conditions of roughly 1atm and 25C, what volume would it occupy?arrow_forward
- In the reaction 2 H2O ==> 2 H2 + O2 the DH = 286 kJ/mole. How much energy (in kJ) must you put in to generate 17.0 Liters of Hydrogen gas (at STP) ?arrow_forwardWhat Is The Ideal-Gas Equation of State?arrow_forwardNatural gas consists primarily of methane, CH4(g).(a) Write a balanced chemical equation for the completecombustion of methane to produce CO2(g) as the onlycarbon-containing product. (b) Write a balanced chemicalequation for the incomplete combustion of methaneto produce CO(g) as the only carbon-containing product.(c) At 25 °C and 1.0 atm pressure, what is the minimumquantity of dry air needed to combust 1.0 L of CH4(g) completelyto CO2(g)?arrow_forward
- How long would it take for 1.50 molmol of water at 100.0 ∘C∘C to be converted completely into steam if heat were added at a constant rate of 20.0 J/sJ/s ?arrow_forwardWhich of the following statement about coal gasification is INCORRECT?A. The synthesis gas is CH4.B. It produces liquid coal under high pressure and temperature.C. It relieves the stress from oil and gas supply.D. It is a type of non-renewable energy.E. The first step is called steam reforming.arrow_forwardWhen limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete — the lime absorbs CO2 from the air and turns back into hard, durable limestone. Suppose a limekiln of volume 300.L is pressurized with carbon dioxide gas to 15.5atm, and heated to 950.0°C. When the amount of CO2 has stopped changing, it is found that 1.79kg of CaCO3 have appeared. Calculate the pressure equilibrium constant Kp this experiment suggests for the equilibrium between CaCO3 and CaO at 950.0°C. Round your answer to 2 significant digits. Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for Kp does not match the accepted value.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
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