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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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Liquid mercury has a density of 13.69 g cm^-3, and solid mercury has a density of 14.690 g cm^-3 both being measured at the melting point, -38.87C, at 1 bar pressure. The heat of fusion is 9.75 J g^-1. Calculate the melting point of mercury at a pressure of 10 bar.
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- Calculate the heat energy released when 22.1 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. Constants for mercury at 1 atm 28.0 heat capacity of Hg(1) melting point enthalpy of fusion J/(mol-K) 234.32 K 2.29 kJ/mol 4p= kJarrow_forwardMercury has a density of 13.69 g/cm3 in the liquid state and 14.193 x 103 kg/m3 in the solid state, both measured at the melting point of 234.33 K at 1 bar. If the heat of fusion of mercury is 9.7876 kJ/kg. What is the melting point of mercury at 7 bar?arrow_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_forward
- The enthalpy of vaporization of a substance is 48.1 kJ/mol. The normal boiling point is 115oC. What is the vapor pressure of this substance at 63.7oC?arrow_forwardAt high altitudes, the ambient air pressure can be significantly less than 1 bar, so water boils at a lower temperature than 100 C. What is the boiling point of water at an altitude where the ambient air pressure is 0.4 bar? The enthalpy of vaporization of water near its boiling point is 40.7 kJ/mol.arrow_forwardWhen 5.00 g of isopropyl alcohol ((CH3),CHOH; molar mass = point of 82.6°C, it absorbs 3.66 kJ of heat. What is the enthalpy of vaporization of isopropyl alcohol in kJ/mol? 60.09 g/mol) evaporates at its boilingarrow_forward
- The vapor pressure of liquid SO, is 281.1 mmHg at a temperature of 242.0 K. The enthalpy of vaporization, AH, What is the vapor pressure of SO2 at a temperature of 250.0 K, in mmHg? for this liquid is 24.9 kJ/mol. чар"arrow_forward. The vapor pressure and enthalpy of vaporization of an unknown substance are measured to be 479.6 torr and 35.3 kJ/mol, respectively at room temperature (298.15 K). Estimate the normal boiling point of the substance at an atmospheric pressure of 760 torr.arrow_forward90. The normal boiling point of water is 100.00 °C and the enthalpy of vaporization at this temperature is ¢vapH = 40.657 kJ mol-1. What would be the boiling point of water if it were based on a pressure of 1 bar instead of the standard atm?arrow_forward
- At high altitudes, the ambient air pressure can be significantly less than 1 bar, so water boils at a lower temperature than 100 C. What is the boiling point of water at an altitude where the ambient air pressure is 0.72 bar? The enthalpy of vaporization of water near its boiling point is 40.7 kJ/mol.arrow_forwardConsider the data in the table. Compound Melting point (°C) AHrus (kJ/mol) Boiling point (°C) AH,ap (kJ/mol) HF -83.11 4.577 19.54 25.18 HCI -114.3 1.991 -84.9 17.53 HBr -86.96 2.406 -67.0 19.27 HI -50.91 2.871 -35.38 21.16 Using the data in the table, calculate ASs and AS for HF. vap ASs = J/(K - mol) ASvap J/(K - mol) Determine the entropy change when 8.40 mol HF(s) melts at atmospheric pressure. AS = J/Karrow_forward
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