43 11.43 How much energy in kilojoules is released when 25.0 g ofethanol vapor at 93.0 °C is cooled to -11.0°C? Ethanol has78.3 °C, AHp4.93 kJ/mol. The molar heat capacity is 112.3J/(K mol) for the liquid and 65.6 J/(K mol) for the vapor.11.44 Draw a molar heating curve for ethanol, C,H,OH, similar to that-114.1 °C, bp38.56 kJ/mol, andmpAHuslonfusic

43) A mole of substance weighs its molar mass and contain avagadro number of particle Let the mass…

How much energy in kilojoules is released when 25.0 g of ethanol vapor at 93.0°C is cooled to -11.0°C? Ethanol has -114.1 °C, bp 78.3 °C, AHap 4.93 kJ/mol. The molar heat capacity is 112.3 38.56 kJ/mol, and mp AHuston 1/(K mol) for the liquid and 65.6 )/(K • mol) for the vapor.

How much energy in kilojoules is released when 25.0 g of ethanol vapor at 93.0°C is cooled to -11.0°C? Ethanol has -114.1 °C, bp 78.3 °C, AHap 4.93 kJ/mol. The molar heat capacity is 112.3 38.56 kJ/mol, and mp AHuston 1/(K mol) for the liquid and 65.6 )/(K • mol) for the vapor.

Introductory Chemistry: A Foundation

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Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

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Problem 17CR: Are changes in state physical or chemical changes? Explain. What type of forces must be overcome to...

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Benzene, C6H6, is an organic liquid that freezes at 5.5 C (Figure 11.1) to form beautiful, feather-like crystals. How much energy is evolved as heat when 15.5 g of benzene freezes at 5.5 C? (The enthalpy of fusion of benzene is 9.95 kJ/mol.) If the 15.5-g sample is remelted, again at 5.5 C, what quantity of energy is required to convert it to a liquid?
1. Which of the following processes requires the largest input of energy as heat? raising the temperature of 100 g of water by 1.0 °C vaporization of 0.10 g of water at 100 °C melting 1.0 g of ice at 0 °C warming 1.0 g of ice from −50 °C to 0 °C (specific heat of ice = 2.06 J/g · K)
The enthalpy change when 1 mol methane (CH4) is burned is 890 kJ. It takes 44.0 kJ to vaporize 1 mol water. What mass of methane must be burned to provide the heat needed to vaporize 1.00 g water?
If you want to convert 56.0 g ice (at 0 °C) to water at 75.0 °C, calculate how many grams of propane, C3H8, you would have to bum to supply the energy to melt the ice and then warm it to the final temperature (at 1 bar).
Equal masses of liquid A, initially at 100C, and liquid B, initially at 50C, are combined in an insulated container. The final temperature of the mixture is 80C. All the heat flow occurs between the two liquids. The two liquids do not react with each other. Is the specific heat of liquid A larger than, equal to, or smaller than the specific heat of liquid B?
Which evolves more heatâ€”freezing 100.0 g of benzene or 100.0 g of bromine?
Sublimation is the phase change from solid to gas without going through a liquid phase. Solid CO2, called dry ice, is an example of one substance that sublimed. Use Hesss law to show that the enthalpy of sublimation, subH, is equal to fusH vapH.
It has been determined that the body can generate 5500 kJ of energy during one hour of strenuous exercise. Perspiration is the bodys mechanism for eliminating this heat. What mass of water would have to be evaporated through perspiration to rid the body of the heat generated during 2 hours of exercise? (The heat of vaporization of water is 40.6 kJ/mol.)
Liquid butane, C4H10, is stored in cylinders to be used as a fuel. Suppose 35.5 g of butane gas is removed from a cylinder. How much heat must be provided to vaporize this much gas? The heat of vaporization of butane is 21.3 kJ/mol.
An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g)+3O2(g)2H2O(l)+2SO2(g);H=1124kJ The density of sulfur dioxide at 25C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/(mol C). (a) How much heat would be evolved in producing 1.00 L of SO2 at 25C and 1.00 atm? (b) Suppose heat from this reaction is used to heat 1.00 L of the SO2 from 25C to 500C for its use in the next step of the process. What percentage of the heat evolved is required for this?
It has been determined that the body can generate 5500 kJ of energy during one hour of strenuous exercise. Perspiration is the body’s mechanism for eliminating this heat. How many grams and how many liters of water would have to be evaporated through perspiration to rid the body of the heat generated during two hours of exercise? (The heat of vaporization of water is 40.6 kJ/mol.)
9.38 The energy densities of various types of coal are listed below: Anthracite 35 kJ/g Subbituminous 31 kJ/g Bituminous 28 kJ/g Lignite 26 kJ/g An unknown sample of one of these coals is burned in an apparatus with a calorimeter constant of 1.3 kJ/°C. When a 0.367-g sample is used, the temperature change is 8.75°C. Which type of coal is the sample?

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