General Chemistry - Standalone book (MindTap Course List)
11th Edition
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
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Chapter 6, Problem 6.14QP
Describe a simple calorimeter. What measurements are needed to determine the heat of reaction?
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Chapter 6 Solutions
General Chemistry - Standalone book (MindTap Course List)
Ch. 6.1 - Prob. 6.1ECh. 6.1 - A solar-powered water pump has photovoltaic cells...Ch. 6.2 - A gas is enclosed in a system similar to that...Ch. 6.2 - Prob. 6.2CCCh. 6.3 - Ammonia burns in the presence of a platinum...Ch. 6.3 - Consider the combustion (burning) of methane, CH4,...Ch. 6.4 - A propellant for rockets is obtained by mixing the...Ch. 6.4 - a. Write the thermochemical equation for the...Ch. 6.4 - Prob. 6.3CCCh. 6.5 - How much heat evolves when 10.0 g of hydrazine...
Ch. 6.6 - Iron metal has a specific heat of 0.449 J/(g+ C)....Ch. 6.6 - Suppose 33 mL of 1.20 M HCl is added to 42 mL of a...Ch. 6.7 - Manganese metal can be obtained by reaction of...Ch. 6.7 - Prob. 6.4CCCh. 6.8 - Calculate the heat of vaporization, Hvap, of...Ch. 6.8 - Prob. 6.12ECh. 6.8 - Calculate the standard enthalpy change for the...Ch. 6 - Define energy, kinetic energy, potential energy,...Ch. 6 - Define the joule in terms of SI base units.Ch. 6 - Prob. 6.3QPCh. 6 - Describe the interconversions of potential and...Ch. 6 - Suppose heat flows into a vessel containing a gas....Ch. 6 - Define an exothermic reaction and an endothermic...Ch. 6 - Prob. 6.7QPCh. 6 - Under what condition is the enthalpy change equal...Ch. 6 - Prob. 6.9QPCh. 6 - Why is it important to give the states of the...Ch. 6 - If an equation for a reaction is doubled and then...Ch. 6 - Prob. 6.12QPCh. 6 - Prob. 6.13QPCh. 6 - Describe a simple calorimeter. What measurements...Ch. 6 - Prob. 6.15QPCh. 6 - You discover that you cannot carry out a...Ch. 6 - Prob. 6.17QPCh. 6 - Prob. 6.18QPCh. 6 - Prob. 6.19QPCh. 6 - Prob. 6.20QPCh. 6 - Is the following reaction the appropriate one to...Ch. 6 - Prob. 6.22QPCh. 6 - Prob. 6.23QPCh. 6 - Prob. 6.24QPCh. 6 - The equation for the combustion of 2 mol of butane...Ch. 6 - A 5.0-g sample of water starting at 60.0C loses...Ch. 6 - Hypothetical elements A2 and B2 react according to...Ch. 6 - Consider the following specific heats of metals....Ch. 6 - Thermal Interactions Part 1: In an insulated...Ch. 6 - Enthalpy a A 100.-g sample of water is placed in...Ch. 6 - Chemical reactions are run in each of the beakers...Ch. 6 - Shown below is a diagram depicting the enthalpy...Ch. 6 - A small car is traveling at twice the speed of a...Ch. 6 - The equation for the combustion of butane, C4H10,...Ch. 6 - A 250-g sample of water at 20.0C is placed in a...Ch. 6 - A 20.0-g block of iron at 50.0C and a 20.0 g block...Ch. 6 - Prob. 6.37QPCh. 6 - A block of aluminum and a block of iron, both...Ch. 6 - You have two samples of different metals, metal A...Ch. 6 - Consider the reactions of silver metal, Ag(s),...Ch. 6 - Prob. 6.41QPCh. 6 - A soluble salt, MX2, is added to water in a...Ch. 6 - Methane, CH4, is a major component of marsh gas....Ch. 6 - Hydrogen sulfide, H2S, is produced during...Ch. 6 - Prob. 6.45QPCh. 6 - Prob. 6.46QPCh. 6 - Chlorine dioxide, ClO2, is a reddish yellow gas...Ch. 6 - Nitrous oxide, N2O, has been used as a dental...Ch. 6 - A gas is cooled and loses 82 J of heat. The gas...Ch. 6 - An ideal gas expands isothermally (at constant...Ch. 6 - The process of dissolving ammonium nitrate,...Ch. 6 - The decomposition of ozone, O3, to oxygen, O2, is...Ch. 6 - Nitric acid, a source of many nitrogen compounds,...Ch. 6 - Hydrogen cyanide is used in the manufacture of...Ch. 6 - What is U when 1.00 mol of liquid water vaporizes...Ch. 6 - What is U for the following reaction at 25C?...Ch. 6 - When 1 mol of iron metal reacts with hydrochloric...Ch. 6 - When 2 mol of potassium chlorate crystals...Ch. 6 - When white phosphorus burns in air, it produces...Ch. 6 - Carbon disulfide burns in air, producing carbon...Ch. 6 - Phosphoric acid, H3PO4, can be prepared by the...Ch. 6 - With a platinum catalyst, ammonia will burn in...Ch. 6 - Colorless nitric oxide, NO, combines with oxygen...Ch. 6 - Hydrogen, H2, is used as a rocket fuel. The...Ch. 6 - Ammonia burns in the presence of a copper catalyst...Ch. 6 - Hydrogen sulfide, H2S, is a foul-smelling gas. It...Ch. 6 - Propane, C3H8, is a common fuel gas. Use the...Ch. 6 - Ethanol, C2H5OH, is mixed with gasoline and sold...Ch. 6 - You wish to heat water to make coffee. How much...Ch. 6 - An iron skillet weighing 1.63 kg is heated on a...Ch. 6 - When steam condenses to liquid water, 2.26 kJ of...Ch. 6 - When ice at 0C melts to liquid water at 0C, it...Ch. 6 - When 15.3 g of sodium nitrate, NaNO3, was...Ch. 6 - When 23.6 g of calcium chloride, CaCl2, was...Ch. 6 - A sample of ethanol, C2H5OH, weighing 2.84 g was...Ch. 6 - A sample of benzene, C6H6, weighing 3.51 g was...Ch. 6 - Hydrazine, N2H4, is a colorless liquid used as a...Ch. 6 - Hydrogen peroxide, H2O2, is a colorless liquid...Ch. 6 - Ammonia will burn in the presence of a platinum...Ch. 6 - Hydrogen cyanide is a highly poisonous, volatile...Ch. 6 - Compounds with carboncarbon double bonds, such as...Ch. 6 - Acetic acid, CH3COOH, is contained in vinegar....Ch. 6 - The cooling effect of alcohol on the skin is due...Ch. 6 - Carbon tetrachloride, CCl4, is a liquid used as an...Ch. 6 - Hydrogen sulfide gas is a poisonous gas with the...Ch. 6 - Carbon disulfide is a colorless liquid. When pure,...Ch. 6 - Iron is obtained from iron ore by reduction with...Ch. 6 - The first step in the preparation of lead from its...Ch. 6 - Hydrogen chloride gas dissolves in water to form...Ch. 6 - Carbon dioxide from the atmosphere weathers, or...Ch. 6 - The Group 2A carbonates decompose when heated. For...Ch. 6 - The Group 2A carbonates decompose when heated. For...Ch. 6 - Prob. 6.93QPCh. 6 - Prob. 6.94QPCh. 6 - Liquid hydrogen peroxide has been used as a...Ch. 6 - Hydrogen is an ideal fuel in many respects; for...Ch. 6 - Niagara Falls has a height of 167 ft (American...Ch. 6 - Prob. 6.98QPCh. 6 - When calcium carbonate, CaCO3 (the major...Ch. 6 - Calcium oxide (quicklime) reacts with water to...Ch. 6 - Formic acid, HCHO2, was first discovered in ants...Ch. 6 - Acetic acid, HC2H3O2, is the sour constituent of...Ch. 6 - Suppose you mix 19.8 g of water at 80.0C with 54.7...Ch. 6 - Suppose you mix 23.6 g of water at 66.2C with 45.4...Ch. 6 - A piece of lead of mass 121.6 g was heated by an...Ch. 6 - The specific heat of copper metal was determined...Ch. 6 - A 44.3 g sample of water at 100.00C was placed in...Ch. 6 - A 19.6-g sample of a metal was heated to 61.67C....Ch. 6 - A 21.3-mL sample of 0.977 M NaOH is mixed with...Ch. 6 - A 29.1-mL sample of 1.05 M KOH is mixed with 20.9...Ch. 6 - In a calorimetric experiment, 6.48 g of lithium...Ch. 6 - When 21.45 g of potassium nitrate, KNO3, was...Ch. 6 - A 10.00-g sample of acetic acid, HC2H3O2, was...Ch. 6 - The sugar arabinose, C5H10O5, is burned completely...Ch. 6 - Hydrogen sulfide, H2S, is a poisonous gas with the...Ch. 6 - Ethylene glycol, HOCH2CH2OH, is used as...Ch. 6 - Hydrogen, H2, is prepared by steam reforming, in...Ch. 6 - Hydrogen is prepared from natural gas (mainly...Ch. 6 - Calcium oxide, CaO, is prepared by heating calcium...Ch. 6 - Sodium carbonate, Na2CO3, is used to manufacture...Ch. 6 - Calculate the heat released when 2,395 L O2 with a...Ch. 6 - Prob. 6.122QPCh. 6 - Sucrose, C12H22O11, is common table sugar. The...Ch. 6 - Prob. 6.124QPCh. 6 - Ammonium nitrate is an oxidizing agent and can...Ch. 6 - Prob. 6.126QPCh. 6 - Prob. 6.127QPCh. 6 - Prob. 6.128QPCh. 6 - Prob. 6.129QPCh. 6 - Prob. 6.130QPCh. 6 - Prob. 6.131QPCh. 6 - Prob. 6.132QPCh. 6 - Dry ice is solid carbon dioxide; it vaporizes at...Ch. 6 - Prob. 6.134QPCh. 6 - Prob. 6.135QPCh. 6 - Sulfur dioxide gas reacts with oxygen, O2(g), to...Ch. 6 - When solid iron burns in oxygen gas (at constant...Ch. 6 - Calculate the grams of oxygen gas required to...Ch. 6 - Hydrogen is burned in oxygen to release heat (see...Ch. 6 - Prob. 6.140QPCh. 6 - Prob. 6.141QPCh. 6 - Prob. 6.142QPCh. 6 - You heat 1.000 quart of water from 25.0C to its...Ch. 6 - A piece of iron was heated to 95.4C and dropped...Ch. 6 - The enthalpy of combustion, H, for benzoic acid,...Ch. 6 - Given the following (hypothetical) thermochemical...Ch. 6 - The head of a strike anywhere match contains...Ch. 6 - Toluene C6H5CH3, has an enthalpy of combustion of...Ch. 6 - What will be the final temperature of a mixture...Ch. 6 - What will be the final temperature of a mixture...Ch. 6 - Graphite is burned in oxygen to give carbon...Ch. 6 - A sample of natural gas is 80.0% CH4 and 20.0%...Ch. 6 - Prob. 6.153QPCh. 6 - Prob. 6.154QPCh. 6 - How much heat is released when a mixture...Ch. 6 - How much heat is released when a mixture...Ch. 6 - Consider the Haber process:...Ch. 6 - An industrial process for manufacturing sulfuric...Ch. 6 - The carbon dioxide exhaled in the breath of...Ch. 6 - A rebreathing gas mask contains potassium...Ch. 6 - Prob. 6.161QP
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- Graphite is burned in oxygen to give carbon monoxide and carbon dioxide. If the product mixture is 33% CO and 67% CO2 by mass, what is the heat from the combustion of 1.00 g of graphite?arrow_forwardHow much heat is released when a mixture containing 10.0 g CS2 and 10.0 g Cl2 reacts by the following equation? CS2(g)+3Cl2(g)S2Cl2(g)+CCl4(g);H=230kJarrow_forwardConsider the following reaction in the vessel described in Question 57. A(g)+B(g)C(s)For this reaction, E=286 J, the piston moves up and the system absorbs 388 J of heat from its surroundings. (a) Is work done by the system? (b) How much work?arrow_forward
- Enthalpy a A 100.-g sample of water is placed in an insulated container and allowed to come to room temperature at 21C. To heat the water sample to 41C, how much heat must you add to it? b Consider the hypothetical reaction,2X(aq)+Y(l)X2Y(aq)being run in an insulated container that contains 100. g of solution. If the temperature of the solution changes from 21C to 31C, how much heat does the chemical reaction produce? How does this answer compare with that in part a? (You can assume that this solution is so dilute that it has the same heat capacity as pure water.) c If you wanted the temperature of 100. g of this solution to increase from 21C to 51C, how much heat would you have to add to it? (Try to answer this question without using a formula.) d If you had added 0.02 mol of X and 0.01 mol of Y to form the solution in part b, how many moles of X and Y would you need to bring about the temperature change described in part c. e Judging on the basis of your answers so far, what is the enthalpy of the reaction 2X(aq) + Y(l) X2Y(aq)?arrow_forwardWhen one mole of ethylene gas, C2H4, reacts with fluorine gas, hydrogen fluoride and carbon tetrafluoride gases are formed and 2496.7 kJ of heat are given off. What is Hf for CF4(g)?arrow_forwardA _________ is a device used to determine the heat associated with a chemical reaction.arrow_forward
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