Introductory Chemistry: A Foundation
8th Edition
ISBN: 9781285199030
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chapter 10, Problem 37QAP
The “Chemistry in Focus” segment Nature Has Hot Plants discusses thermogenic, or heat-producing, plants. For some plants, enough heat is generated to increase the temperature of the blossom by 15 °C. About how much heat is required to increase the temperature of 1 L of water by 15 °C?
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Chapter 10 Solutions
Introductory Chemistry: A Foundation
Ch. 10.1 - at if energy were not conserved? How would this...Ch. 10.4 - u are calculating in a chemistry problem. What if...Ch. 10.5 - ercise 10.1 How many calories of energy correspond...Ch. 10.5 - ercise 10.2 Calculate the joules of energy...Ch. 10.5 - ercise 10.3 A 5.63-g sample of solid gold is...Ch. 10.5 - ercise 10.4 A 2.8-g sample of pure metal requires...Ch. 10.6 - Prob. 10.5SCCh. 10.7 - at if Hess’s law were not true? What are some...Ch. 10.7 - Prob. 10.6SCCh. 10.9 - Prob. 1CT
Ch. 10.10 - at if the first law of thermodynamics was true,...Ch. 10 - Prob. 1ALQCh. 10 - friend of yours reads that the process of water...Ch. 10 - ou place hot metal into a beaker of cold water. ol...Ch. 10 - Prob. 4ALQCh. 10 - Prob. 5ALQCh. 10 - xplain why aluminum cans make good storage...Ch. 10 - n Section 10.7, two characteristics of enthalpy...Ch. 10 - Prob. 8ALQCh. 10 - hat is meant by the term driving forces? Why are...Ch. 10 - Prob. 10ALQCh. 10 - Explain in your own words what is meant by the...Ch. 10 - Prob. 12ALQCh. 10 - What if energy was not conserved? How would this...Ch. 10 - The internal energy of a system is said to be the...Ch. 10 - Hydrogen gas and oxygen gas react violently to...Ch. 10 - Consider four 100.0-g samples of water, each in a...Ch. 10 - For each of the following situations ac. use the...Ch. 10 - Prob. 18ALQCh. 10 - Does the entropy of the system increase or...Ch. 10 - Prob. 20ALQCh. 10 - Prob. 1QAPCh. 10 - Prob. 2QAPCh. 10 - Prob. 3QAPCh. 10 - Prob. 4QAPCh. 10 - Prob. 5QAPCh. 10 - n Fig. 10.1, what kind of energy does ball A...Ch. 10 - Prob. 7QAPCh. 10 - f you spilled a cup of freshly brewed hot tea on...Ch. 10 - Prob. 9QAPCh. 10 - Prob. 10QAPCh. 10 - In studying heat flows for chemical processes,...Ch. 10 - When a chemical system evolves energy, where does...Ch. 10 - The combustion of methane, is an exothermic...Ch. 10 - Are the following processes exothermic or...Ch. 10 - What do we mean by thermodynamics? What is the...Ch. 10 - Prob. 16QAPCh. 10 - Calculate A£ for each of the following cases q =...Ch. 10 - If q for a process is a positive number, then the...Ch. 10 - For an endothermic process, q will have a...Ch. 10 - A system releases 125 kJ of heat and 104 kJ of...Ch. 10 - Prob. 21QAPCh. 10 - Prob. 22QAPCh. 10 - If 8.40 kJ of heat is needed to raise the...Ch. 10 - If it takes 654 J of energy to warm a 5.51-g...Ch. 10 - Prob. 25QAPCh. 10 - Prob. 26QAPCh. 10 - Covert the following numbers of kilojoules into...Ch. 10 - Prob. 28QAPCh. 10 - Prob. 29QAPCh. 10 - Prob. 30QAPCh. 10 - .5 kJ of heat is applied to a 1012-g block of...Ch. 10 - What quantity of heat energy must have en applied...Ch. 10 - If 125 J of heat energy is applied to a block of...Ch. 10 - If 100. J of heat energy is applied to a 25-g...Ch. 10 - What quantity of heat is required to raise the...Ch. 10 - Prob. 36QAPCh. 10 - The “Chemistry in Focus” segment Nature Has Hot...Ch. 10 - In the “Chemistry in Focus” segment Firewalking:...Ch. 10 - Prob. 39QAPCh. 10 - A _________ is a device used to determine the heat...Ch. 10 - The enthalpy change for the reaction of hydrogen...Ch. 10 - For the reaction kJ per mole of formed. Calculate...Ch. 10 - Prob. 43QAPCh. 10 - When ethanol (grain alcohol, is burned in oxygen,...Ch. 10 - Prob. 45QAPCh. 10 - Prob. 46QAPCh. 10 - Prob. 47QAPCh. 10 - Prob. 48QAPCh. 10 - Prob. 49QAPCh. 10 - Prob. 50QAPCh. 10 - Prob. 51QAPCh. 10 - Prob. 52QAPCh. 10 - Prob. 53QAPCh. 10 - Prob. 54QAPCh. 10 - Prob. 55QAPCh. 10 - Prob. 56QAPCh. 10 - Prob. 57QAPCh. 10 - Prob. 58QAPCh. 10 - Prob. 59QAPCh. 10 - Prob. 60QAPCh. 10 - If a reaction occurs readily but has an...Ch. 10 - Prob. 62QAPCh. 10 - Prob. 63QAPCh. 10 - Prob. 64QAPCh. 10 - Prob. 65APCh. 10 - Calculate the enthalpy change when 1.0(1 g of...Ch. 10 - Prob. 67APCh. 10 - Calculate the amount of energy required (in...Ch. 10 - If takes 1.25 kJ of energy to heat a certain...Ch. 10 - What quantity of heat energy would have to be...Ch. 10 - The specific heat capacity of gold is 0.13 J/g °C....Ch. 10 - Calculate the amount of energy required (in...Ch. 10 - If 10. J of heat is applied to 5.0-g samples of...Ch. 10 - A 50.1)-g sample of water at 100. °C is poured...Ch. 10 - A 25.0-g sample of pure iron at 85 °C is dropped...Ch. 10 - If 7.24 kJ of heat is applied to a 952-g block of...Ch. 10 - For each of the substances listed in Table 10.1,...Ch. 10 - A system releases 213 kJ of heat and has a...Ch. 10 - Prob. 79APCh. 10 - Calculate the enthalpy change when 5.00 g of...Ch. 10 - Prob. 81APCh. 10 - Prob. 82APCh. 10 - It has been determined that the body can generate...Ch. 10 - Prob. 84APCh. 10 - Prob. 85CPCh. 10 - The specific heat capacity of graphite is 0.71 J/g...Ch. 10 - A swimming pool, 10.0 in by 4.0 m, is filled with...Ch. 10 - Prob. 88CPCh. 10 - Prob. 89CP
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- 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_forwardIf 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?arrow_forwardA rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.arrow_forward
- You are camping and contemplating placing some hot objects into your sleeping bag to warm it. You warm a rock and a canteen of water, of roughly equal mass, around the fire. Which would be more effective in warming your sleeping bag? Why?arrow_forwardA 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_forwardIf 125 J of heat energy is applied to a block of silver weighing 29.3 g, by how many degrees will the temperature of the silver increase? (See Table 10.1.)arrow_forward
- The equation for the fermentation of glucose to alcohol and carbon dioxide is: C6H12O6(aq) 2C2H5OH(aq) + 2CO2(g) The enthalpy change for the reaction is 67 kJ. Is this reaction exothermic or endothermic? Is energy, in the form of heat, absorbed or evolved as the reaction occurs?arrow_forwardDetermine whether the statements given below are true or false. Consider an endothermic process taking place in a beaker at room temperature. (a) Heat flows from the surroundings to the system. (b) The beaker is cold to the touch. (c) The pressure of the system decreases. (d) The value of q for the system is positive.arrow_forwardHow much heat is evolved when 1255 g of water condensesto a liquid at 100°C?arrow_forward
- Copper is used in building the integrated circuits, chips, and printed circuit boards for computers. When 228 J of heat are absorbed by 125 g of copper at 22.38C, the temperature rises to 27.12C. What is the specific heat of copper?arrow_forwardIs the Sun exothermic or endothermic? Is it any less exothermic or endothermic in the winter, as opposed to the summer?arrow_forwardA piece of chocolate cake contains about 400 calories. A nutritional calorie is equal to 1000 calories (thermochemical calories), which is equal to 4.184 kJ. How many 8-in-high steps must a 180-lb man climb to expend the 400 Cal from the piece of cake? See Exercise 28 for the formula for potential energy.arrow_forward
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