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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text:From the following vapor pressure data for ethanol, an estimate of the molar heat of vaporization of C,H;OH is
kJ/mol.
P, mm Hg T, Kelvins
308
337
100
400
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- The heat of fusion for a material can be found by AHfus = m x Cp x AT where AHfus is the heat of fusion per gram, m is the mass of the solid substance being melted, C, is the specific heat of the surrounding medium, and ATis the change in the temperature of the surrounding medium as the solid melts. Calculate the heat of fusion of a 10.00-g piece of Substance X. Use 4.18 J/g-° C as the specific heat, and assume a AT of 10.00 °C. Express your answer to three significant figures (units of J/g) 41.8 418 O 4.18arrow_forwardWhat quantity of heat is required to convert 19.0 g of ethanol (C₂H₅OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (heat capacity of ethanol = 2.46 J/g • C; ∆Hvap = 39.3 kJ/mol)arrow_forwardTwo 20.0 g ice cubes at -17.0 °C are placed into 235 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/ (mol·K) heat capacity of H,O(1) 75.3 J/ (mol·K) T = enthalpy of fusion of H,O 6.01 kJ/molarrow_forward
- Octane(C3H18) is a hydrocarbon found in crude oil. Thermochemical data for octane is provided below. The total change in enthalpy is 15.94 kJ when heating 0.2500 moles of octane from -70.00°C to 100.0°C. Determine the AHfusion. Melting point: -57.00 °C Boiling point: 126.0 °C J Csolid : 185.0 °C mol J Cliquid: 254.0 °C mol J Cgas: 250.0 °C mol AHvap: 34.40 kJ/ mol Molar mass: 114.23 g/mol 0.2693 kJ/mol 4.720 kJ/mol O 21.50 kJ/mol 0.2540 J/molarrow_forwardAn ice cube with a mass of 45.4 g at 0.0 °C is added to a glass containing 374 g of water at 45.0 °C. Determine the final temperature of the system at equilibrium. The specific heat capacity of water, C, is 4.184 J/g.°C, and the standard enthalpy of fusion, AH; , of water is 6.01 × 10° J/mol. Assume that no energy is transferred to or from the surroundings. fus T = °C TOOLS x10 Question Source: Atkins 7e - Chemical Principles| Publisher: W.H. Frearrow_forwardTwo 20.0 g ice cubes at –16.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, T;, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/(mol·K) Tf = heat capacity of H,O(l) 75.3 J/(mol-K) enthalpy of fusion of H,O 6.01 kJ/molarrow_forward
- instant pan pressure cooker has an enthalpy of vaporization of water 40.67 kJ/mole. calculate the boiling temperature C of water inside a pressure pan cooker that has been pressurized to 5.9 atm.arrow_forwardA substance has the following properties: AHfus 10.0 kJ/mol AHvap=20.0 kJ/mol Cp (solid) = 60. J mol-¹ K-¹ Cp (liquid) = 30. J mol-¹ K-¹ Cp (gas) = 60. J mol-¹ K-¹ =arrow_forwardCalculate the heat change in joules for vaporization of 9.00 g of water at 100 ∘C.arrow_forward
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