help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working empts/There is no attempt penalty05 Question (1 point)e See section 17.2It takes 38.6 kJ of energy to vaporize 1.00 mol of ethanol (MW: 46.07 g/mol). What will be AS sys for the vaporization of 3.50 g of ethanol at 79.2 °C?1st attemptAS-J/KSee Periodic Table

To find the entropy change (Δ𝑆sysΔS sys) for the vaporization of ethanol at 79.2°C, we need to use…

empts/There is no attempt penalty 05 Question (1 point) e See section 17.2 It takes 38.6 kJ of energy to vaporize 1.00 mol of ethanol (MW: 46.07 g/mol). What will be AS sys for the vaporization of 3.50 g of ethanol at 79.2 °C? 1st attempt AS- J/K See Periodic Table

empts/There is no attempt penalty 05 Question (1 point) e See section 17.2 It takes 38.6 kJ of energy to vaporize 1.00 mol of ethanol (MW: 46.07 g/mol). What will be AS sys for the vaporization of 3.50 g of ethanol at 79.2 °C? 1st attempt AS- J/K See Periodic Table

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 81E: Given the following data...

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9.86 You make some iced tea by dropping 134 g of ice into 500.0 mL of warm tea in an insulated pitcher. If the tea is initially at 20.0°C and the ice cubes are initially at 0.0°C, how many grams of ice will still be present when the contents of the pitcher reach a final temperature? The tea is mostly water, so assume that it has the same density (1.0 g/mL), molar mass, heat capacity (75.3 J K-1 mol-1), and heat of fusion (6.0 kJ/mol) as pure water. The heat capacity of ice is 37.7 J K-l mol-l.
Given the following data Fe2O3(s)+3CO(g)2Fe(s)+3CO2(g)H=23KJ3Fe2O3(s)+CO(g)2Fe3O4(s)+CO2(g)H=39KJFe3O4(s)+CO(g)3FeO(s)+CO2(g)H=18KJ Calculate H for this reaction FeO(s)+CO(g)Fe(s)+CO2(g)
Choose the substance with the larger positional probability in each case. a. 1 mole of H2 (at STP) or 1 mole of H2 (at l00C, 0.5 atm) b. 1 mole of N2 (at STP) or 1 mole of N2 (at l00 K, 2.0 atm) c. 1 mole of H2O(s) (at 0C) or 1 mole of H2O(l) (at 20C)
The combustion of methane can be represented as follows: a. Use the information given above to determine the value of H for the combustion of methane to form CO2(g) and 2H2O(l). b. What is Hf for an element in its standard state? Why is this? Use the figure above to support your answer. c. How does H for the reaction CO2(g) + 2H2O (1) CH4(g) + O2(g) compare to that of the combustion of methane? Why is this?
Some automobiles and buses have been equipped to bum propane (C3H8). Compare the amounts of energy that can be obtained per gram of C3H8(g) and per gram of gasoline, assuming that gasoline is pure octane, C8H18(l). (See Example 7-11.) Look up the boiling point of propane. What disadvantages are there to using propane instead of gasoline as a fuel?
Calculate H for the reaction 2NH3(g)+12O2(g)N2H4(l)+H2O(l) given the following data: 2NH3(g)+3N2O(g)4N2(g)+3H2O(l)H=1010.KJN2O(g)+3H2(g)N2H4(l)+H2O(l)H=317KJN2H4(l)+O2(g)N2(g)+2H2O(l)H=623KJH2(g)+12O2(g)H2O(l)H=286KJ
A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at room temperature (22.5C) to vapor at 59.0C.To do this, one must use Tables 8.1 and 8.2 for information on the specific heat, boiling point, and heat of vaporization of bromine. In addition, the following step-wise process must be followed. (a) Calculate H for: Br2(l,22.5C)Br2(l,59.0C) (b) Calculate H for: Br2(l,59.0C)Br2(g,59.0C) (c) Using Hess's law, calculate H for: Br2(l,22.5C)Br2(g,59.0C)
Strontium metal is responsible for the red color in fireworks. Fireworks manufacturers use strontium carbonate, which can be produced by combining strontium metal, graphite (C), and oxygen gas. The formation of one mole of SrCO3 releases 1.220103 kJ of energy. (a) Write a balanced thermochemical equation for the reaction. (b) What is H when 10.00 L of oxygen at 25C and 1.00 atm are used by the reaction?
9.103 One reason why the energy density of a fuel is important is that to move a vehicle one must also move its unburned fuel. Octane is a major component of gasoline. It burns according to the reaction 2C8H18(l)+25O2(g)16CO2(g)+18H2O(g) H = 1.10104 kJ Starting from this thermochemical equation, describe how you would determine the energy density, in kJ/g, for octane. Be sure to indicate what you would need to calculate or look up to complete this problem.
9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.
9.47 If 14.8 kJ of heat is given off when 1.6 g of HCl condenses from vapor to liquid, what is Hcond for this substance?
9.91 You want to heat the air in your house with natural gas (CH4). Assume your house has 275 m2(ahout 2800 ft2) of floor area and that the ceilings are 2.50 m from the floors. The air in the house has a molar heat capacity of 29.1 J mol-l K-l. (The number of moles of air in the house may he found by assuming that the average molar mass of air is 28.9 g/mol and that the density of air at these temperatures is 1.22 g/L.) What mass of methane do you have to burn to heat the air from 15.0 to 22.0°C?

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