Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- What amount of thermal energy (in kJ) is required to convert 38.2 g of ethanol at -148 °C completely to gaseous ethanol at 100 °C? The melting point of ethanol is -114 °C and its normal boiling point is 78 °C. The heat of fusion of ethanol is 5.0 kJ mol-1 The heat of vaporization of ethanol at its normal boiling point is 35.0 kJ mol-¹ The specific heat capacity of solid ethanol is 1.05 J g-¹ °C-1 The specific heat capacity of liquid ethanol is 2.44 J g-¹ °C-¹ The specific heat capacity of gaseous ethanol is 1.01 J g-¹ °C-¹ Answer:arrow_forwardCalculate the amount of energy (in kJ) necessary to convert 497 g of liquid water from 0°C to water vapor at 182°C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g °C, and for steam is 1.99 J/g °C. (Assume that the specific heat values do not change over the range of temperatures in the problem.) kJarrow_forwardCalculate the energy released as heat when 18.7 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. heat capacity of Hg(1) Constants for mercury at 1 atm melting point enthalpy of fusion 28.0 J/(mol-K) # 234.32 K 2.29 kJ/mol 9 = MacBook Proarrow_forward
- What amount of thermal energy (in kJ) is required to convert 221 g of ice at -16 °C completely to water vapour at 214 °C? The melting point of water is 0 °C and its normal boiling point is 100 °C. The heat of fusion of water is 6.02 kJ mol-¹ The heat of vaporization of water at its normal boiling point is 40.7 kJ mol-¹ The specific heat capacity of ice is 2.09 J g-¹ °C-¹ The specific heat capacity of liquid water is 4.18 J g-¹ °C-¹ The specific heat capacity of water vapour is 2.01 Jg¹¹ °C-¹ Answer:arrow_forwardCalculate the heat required to convert 22.2 g of propyl alcohol, C3H3O, from a solid at -141°C into the gaseous state at 115°C. The normal melting and boiling points of this substance are -127°C and 97°C, respectively. The heat of fusion is 86.2 J/g, and the heat of vaporization is 694 J/g. The specific heats of the solid, liquid and gaseous states are, respectively, 2.36, 2.83 and 1.76 J/g/K.arrow_forwardEthanol (C₂H₂OH) meits at-114 °C and boils at 78°C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 and 2.3 J/(g-K), respectively. Y Part A How much heat is required to convert 30.5 g of ethanol at 28 °C to the vapor phase at 78 "C? Express your answer in kilojoules to three significant figures. 195] ΑΣΦ Submit Part 8 Request Answer Submit ? How much heat is required to convert 30.5 g of ethanol at-160 C to the vapor phase at 78 "C7 Express your answer in kilojoules to two significant figures. VA24 Request Answer kJ kJarrow_forward
- Please explain step by step (it would be helpful if you also graph it)arrow_forwardWith around 70% of ammonia produced industrially being used to make fertilizers. The specific heat capacity of liquid ammonia is 80.8 J/g*K while that of gaseous ammonia is 37.0 J/g*K. Given that the boiling point and enthalpy of vaporization of ammonia is -33.3°C and 23.5 kJ/mol, respectively, how much energy is required to heat 75 g of ammonia (17.03 g/mol) from the temperature of liquid nitrogen (-195.8°C) to room temperature (25.0°C)?arrow_forwardHow much heat energy is required to convert 44.9 g of solid ethanol at -114.5 °C to gasesous ethanol at 160.8 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol, and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of –114.5°C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45J/g · °C, and that of gaseous ethanol is 1.43J/g · °C. kJarrow_forward
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