EBK CHEMISTRY: THE MOLECULAR NATURE OF
7th Edition
ISBN: 9781119513216
Author: HYSLOP
Publisher: JOHN WILEY+SONS INC.
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Textbook Question
Chapter 6, Problem 53RQ
How much heat, in joules and in calories, must be removed from 1.75 mol of water to lower its temperature
from
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When 0.800 grams of NaOH is dissolved in 100.0 grams of water, the temperature of the solution increases from 25.00 °C to 27.06 °C. What is the amount of heat absorbed by the water in joules? The specific heat of water is 4.18 J/g•°C.
The salt calcium chloride is soluble in water. When 1.14 g of CaCl2 is dissolved in 115.00 g of water, the temperature of the solution increases from 25.00 to 26.82 °C. Based on this observation, calculate the enthalpy of dissolution of CaCl2 (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible.
11. When 6.50 g of solid NaOH is dissolved in 100,0 g of water in a calorimeter, the
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in kJ/mol of NaOH, Assume specific heat of solution is the same as water.
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Chapter 6 Solutions
EBK CHEMISTRY: THE MOLECULAR NATURE OF
Ch. 6 - Prob. 1PECh. 6 - Prob. 2PECh. 6 - When monitoring a reaction, the initial...Ch. 6 - Practice Exercise 6.4
A hall bearing at is...Ch. 6 - Prob. 5PECh. 6 - Silicon, used in computer chips, has a specific...Ch. 6 - Would the explosive reaction of hydrogen and...Ch. 6 - Practice Exercise 6.8
When ammonium nitrate is...Ch. 6 - An exothermic reaction is carried out at a...Ch. 6 - For an exothermic reaction that is conducted under...
Ch. 6 - Since it can be obtained in very high purity,...Ch. 6 - A 1.50 g sample of pure sucrose is burned in a...Ch. 6 - For the Analyzing and Solving Multi-Concept...Ch. 6 - Practice Exercise 6.14
The exact same procedure as...Ch. 6 - The combustion of methane can be represented by...Ch. 6 - Practice Exercise 6.16
What is the thermochemical...Ch. 6 - Two oxides of copper can be made from copper by...Ch. 6 - Consider the following thermochemical...Ch. 6 - Given the following thermochemical equations,...Ch. 6 - Ethanol, C2H5OH, is made industrially by the...Ch. 6 - Practice Exercise 6.21
The heat of combustion, ,...Ch. 6 - Practice Exercise 6.22
n-Octane, , has a standard...Ch. 6 - Write the thermochemical equation that would be...Ch. 6 - Write the thermochemical equation that would be...Ch. 6 - Use heats of formation data from Table 6.2 to...Ch. 6 - Write thermochemical equations corresponding to Hf...Ch. 6 - Calculate H for the following reactions:...Ch. 6 - Give definitions for (a) energy, (b) kinetic...Ch. 6 - Prob. 2RQCh. 6 - Prob. 3RQCh. 6 - 6.4 State the law of conservation of energy....Ch. 6 - 6.5 A pendulum such as a swinging chandelier...Ch. 6 - Prob. 6RQCh. 6 - 6.7 What is meant by the term chemical energy?
Ch. 6 - How does the potential energy change (increase,...Ch. 6 - What is the SI unit of energy? How much energy (in...Ch. 6 - 6.10 Why is hear considered a waste product in a...Ch. 6 - Prob. 11RQCh. 6 - 6.12 How is internal energy related to molecular...Ch. 6 - On a molecular level, how is thermal equilibrium...Ch. 6 - Consider the distribution of molecular kinetic...Ch. 6 - Suppose the temperature of an object is raised...Ch. 6 - A quart of boiling water will cause a more severe...Ch. 6 - Prob. 17RQCh. 6 - What is a state function? Give four examples that...Ch. 6 - How would you determine whether an experimental...Ch. 6 - 6.20 How can the state of a system be specified?
Ch. 6 - 6.21 What do the terms system and surroundings...Ch. 6 - What are the names of the thermal properties whose...Ch. 6 - 6.23 For samples with the same mass, which kind of...Ch. 6 - 6.24 How do heat capacity and specific hear...Ch. 6 - Prob. 25RQCh. 6 - 6.26 Suppose object A has twice the specific heat...Ch. 6 - In a certain chemical reaction, there is a...Ch. 6 - 6.28 What term do we use to describe a reaction...Ch. 6 - 6.29 What term is used to describe a reaction that...Ch. 6 - 6.30 When gasoline burns, it reacts with oxygen in...Ch. 6 - Write the equation that states the first law of...Ch. 6 - How are heat and work defined?Ch. 6 - Devise an example, similar to the one described in...Ch. 6 - 6.34 Why are heat and work not state functions?
Ch. 6 - When we measure the heat of combustion of glucose,...Ch. 6 - Consider the reaction...Ch. 6 - How is enthalpy defined?Ch. 6 - What is the sign of H for an endothermic change?Ch. 6 - 6.39 If the enthalpy of a system increases by 100...Ch. 6 - If a system containing gases expands and pushes...Ch. 6 - 6.41 Why do standard reference values for...Ch. 6 - What distinguishes a thermochemical equation from...Ch. 6 - Why are fractional coefficients permitted in a...Ch. 6 - 6.44 What fundamental fact about makes Hess’s law...Ch. 6 - 6.45 What two conditions must be met by a...Ch. 6 - Describe what must be done with the standard...Ch. 6 - What two additional thermochemical equations are...Ch. 6 - Peptides, small parts of proteins, contain...Ch. 6 - If a car increases its speed from 30 mph to 60...Ch. 6 - 6.50 If the mass of a truck is doubled—for...Ch. 6 - 6.51 What is the kinetic energy, in joules, of a...Ch. 6 - What is the kinetic energy, in joules, of a...Ch. 6 - How much heat, in joules and in calories, must be...Ch. 6 - 6.54 How much heat, in joules and calories, is...Ch. 6 - How many grams of water can be heated from...Ch. 6 - 6.56 How many grams of copper can be cooled from ...Ch. 6 - A 50.0 g piece of a metal at 100.0C was plunged...Ch. 6 - 6.58 A sample of copper was heated to and then...Ch. 6 - 6.59 Calculate the molar heat capacity of iron in...Ch. 6 - 6.60 What is the molar heat capacity of ethyl...Ch. 6 - A vat of 4.54 kg of water underwent a decrease in...Ch. 6 - A container filled with 2.46 kg of water underwent...Ch. 6 - 6.63 Nitric acid neutralizes potassium hydroxide....Ch. 6 - In the reaction between formic acid (HCHO2) and...Ch. 6 - 6.65 A 1.000 mol sample of propane, a gas used for...Ch. 6 - Toluene, C7H8, is used in the manufacture of...Ch. 6 - If a system does 4$ J of work and receives 28 J of...Ch. 6 - If a system has 48 J of work done on it and...Ch. 6 - An automobile engine converts heat into work via a...Ch. 6 - Chargers for cell phones get warm while they are...Ch. 6 - If the engine in Problem 6.69 absorbs 250 joules...Ch. 6 - If a battery can release 535 J of energy and 455 J...Ch. 6 - Ammonia reacts with oxygen as follows:...Ch. 6 - One thermochemical equation for the reaction of...Ch. 6 - Magnesium bums in air to produce a bright light...Ch. 6 - Methanol is the fuel in canned heat containers...Ch. 6 - Methane burns with oxygen to produce carbon...Ch. 6 - Methanol, as described in Problem 6.76, is used to...Ch. 6 - *6.79 Construct an enthalpy diagram that shows the...Ch. 6 - *6.80 Construct an enthalpy diagram for the...Ch. 6 - Show how the equations...Ch. 6 - 6.82 We can generate hydrogen chloride by heating...Ch. 6 - Calculate H in kilojoules for the following...Ch. 6 - Calcium hydroxide reacts with hydrochloric acid by...Ch. 6 - Given the following thermochemical equations,...Ch. 6 - 6.86 Given the following thermochemical...Ch. 6 - Given the following thermochemical equations,...Ch. 6 - Given the following thermochemical equations,...Ch. 6 - Which of the following thermochemical equations...Ch. 6 - Which of the following thermochemical equations...Ch. 6 - Write the thermochcmical equations, including...Ch. 6 - Write the thermochemical equations, including...Ch. 6 - Using data in Table 6.2, calculate H in kilojoules...Ch. 6 - 6.94 Using data in Table 6.2, calculate in...Ch. 6 - The value for the standard heat of combustion, H...Ch. 6 - The thermochemical equation for the combustion of...Ch. 6 - 6.97 Look at the list of substances in Table 6.1....Ch. 6 - *6.98 A dilute solution of hydrochloric acid with...Ch. 6 - A 2.00 kg piece of granite with a specific heat of...Ch. 6 - In the recovery of iron from iron ore, the...Ch. 6 - Use the results of Problem 6.100 and the data in...Ch. 6 - 6.102 The amino acid glycine, , is one of the...Ch. 6 - The value of Hf for HBr(g) was first evaluated...Ch. 6 - Acetylene, C2H2, is a gas commonly burned in...Ch. 6 - The reaction for the metabolism of sucrose,...Ch. 6 - Consider the following thermochemical...Ch. 6 - 6.107 Chlorofluoromethanes (CFMs) are carbon...Ch. 6 - Prob. 108RQCh. 6 - Suppose a truck with a mass of 14.0 tons...Ch. 6 - How much work must be done to form one mole of CH4...Ch. 6 - A cold -15C piece of copper metal weighing 7.38 g...Ch. 6 - Both Na2CO3 and NaHCO3 can be used to neutralize...Ch. 6 - *6.113 When 4.56 g of a solid mixture composed of ...Ch. 6 - Using the results from Analyzing and Solving...Ch. 6 - *6.115 For ethanol, , which is mixed with gasoline...Ch. 6 - Both calcium and potassium react with water to...Ch. 6 - 6.117 As a routine safety procedure, acids and...Ch. 6 - In an experiment, 95.0 mL of 0.225 M silver...Ch. 6 - 6.119 Growing wheat and converting it into bread...Ch. 6 - Suppose we compress a spring, tie it up tightly,...Ch. 6 - Prob. 121RQCh. 6 - Why do we usually use H rather than E when we...Ch. 6 - Prob. 123RQCh. 6 - 6.124 Find the heats of formation of some...Ch. 6 - Prob. 125RQ
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- A student used a coffee-cup calorimeter to determine the enthalpy of solution for NH4NO3.When NH4NO3 is added to water, there is a decrease in temperature of the solution. Is the solution process exothermic or endothermic? (a) endothermic (b) exothermicarrow_forwardAre changes in state physical or chemical changes? Explain. What type of forces must be overcome to melt or vaporize a substance (are these forces intramolecular or intermolecular)? Define the molar heat of fusion and molar heat of vaporization. Why is the molar heat of vaporization of water so much larger than its molar heat of fusion? Why does the boiling point of a liquid vary with altitude?arrow_forwardHow much heat, in joules and in calories, must be added to a 75.0g iron block with a specific heat of 0.449 Jig C to increase its temperature from 25 C to its melting temperature of 1535 C?arrow_forward
- How much would the temperature of 275 g of water increase if 36.5 U of heat were added?arrow_forwardEnthalpy 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_forwardA 0.500-g sample of KCl is added to 50.0 g of water in a calorimeter (Figure 5.12). If the temperature decreases by 1.05 °C, what is the approximate amount of heat involved in the dissolution of the KCl, assuming the specific heat of the resulting solution is 4.18 J/g °C? Is the reaction exothermic or endothermic?arrow_forward
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