Learning Goal:To calculate the total energy required to convert a solid to agas using heat capacity, heat of fusion, and heat ofvaporization.The amount of heat required to melt one mole of a solid iscalled the heat of fusion (AHfus). The amount of heatrequired to vaporize (boil) one mole of a liquid is called theheat of vaporization (AHvap). The heat of fusion and theheat of vaporization can be used to calculate the amount ofheat needed to melt or vaporize, respectively, a given amountof substance.For example, the heat of fusion for H2O is 6.02 kJ/mol,which means that 6.02 kJ of heat is needed to melt a mole ofice. Twice as much heat is needed to melt twice as much ice,as shown here:2.00 mol x 6.02 kJ/mol = 12.0 kJ%3DPart CHow much heat is required to boil 81.5 g of water at its boiling point?Express your answer numerically in kilojoules.> View Available Hint(s)kJ

Mass of water = 81.5 g Boiling point of water = 1000C ∆Hvap = 40.7 kJ/mol

To calculate the total energy required to convert a solid to gas using heat capacity, heat of fusion, and heat of vaporization. The amount of heat required to melt one mole of a solid is called the heat of fusion (AHfus). The amount of heat required to vaporize (boil) one mole of a liquid is called the heat of vaporization (AHvap). The heat of fusion and the heat of vaporization can be used to calculate the amount o heat needed to melt or vaporize, respectively, a given amoI of substance. For example, the heat of fusion for H2O is 6.02 kJ/mol, which means that 6.02 kJ of heat is needed to melt a mole ice. Twice as much heat is needed to melt twice as much ice as shown here: 2.00 mol x 6.02 kJ/mol = 12.0 kJ %3D

To calculate the total energy required to convert a solid to gas using heat capacity, heat of fusion, and heat of vaporization. The amount of heat required to melt one mole of a solid is called the heat of fusion (AHfus). The amount of heat required to vaporize (boil) one mole of a liquid is called the heat of vaporization (AHvap). The heat of fusion and the heat of vaporization can be used to calculate the amount o heat needed to melt or vaporize, respectively, a given amoI of substance. For example, the heat of fusion for H2O is 6.02 kJ/mol, which means that 6.02 kJ of heat is needed to melt a mole ice. Twice as much heat is needed to melt twice as much ice as shown here: 2.00 mol x 6.02 kJ/mol = 12.0 kJ %3D

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

How much energy is required to heat 17.1 g acetone (MM = 58.08 g/mol) from a solid at -114.0°C to a liquid at -27.0°C? The following physical data may be useful.ΔHfus = 7.27 kJ/molSpecific Heat - liquid = 2.16 J/g°CSpecific Heat - Gas = 1.29 J/g°CSpecific Heat - Solid = 1.6
What amount of heat (in kJ) is required to convert 30.0 g of an unknown solid (MM = 67.44 g/mol) at -15.4 °C to a liquid at 42.7 °C? (specific heat capacity of solid = 1.95 J/g･°C; specific heat capacity of liquid = 1.18 J/g･°C; ∆Hfus = 5.72 kJ/mol; normal freezing point, Tf = 28.3°C)
Liquid ammonia (boiling point = –4°C) can be used as a refrigerant and heat transfer fluid. How much energy is needed to heat 25.0 g of NH3(l) from –65.0°C to –12.0°C? Specific heat, NH3 (l) 4.7 J/g K Specific heat, NH3 (g) 2.2 J/g K Heat of vaporization 23.5 kJ/mol
Two 20.0 g ice cubes at -17.00C are placed into 470.1 g of water at 25.0 0C. The heat of fusion of ice is 6.008 kJ/mol, the molar heat capacity of water is 75.3 J mol-1 K-1 and the molar heat capacity of ice is 37.7 J mol-1 K-1. Assuming no energy is transferred to or from the surroundings, please calculate the final temperature of the water after all the ice melts. _______ 0C
You may want to reference Section 3.7 (Pages 80 - 87) while completing this problem.Using the values for the heat of fusion, specific heat of water, and/or heat of vaporization, calculate the amount of heat energy in each of the following. Keep in mind that the sign of the heat involved in the state change is ignored.Part ACalculate the joules released when 175 g of the steam condenses at 100 ∘C and the liquid cools to 35.0 ∘C.
The following information is given for ethanol at 1 atm: Boiling point = 78.40°C Melting point =-114.5°C Specific heat gas = 0.3418 cal/g°C Specific heat liquid = 0.5880 cal/g°C Heat of vaporization = 200.0 cal/g Heat of fusion = 26.04 cal/g A 44.00 g sample of liquid ethanol is initially at -58.80°C. How many kcal of energy must be added to the sample to raise its temperature to 94.90°C? Energy added = kcal
Calculate 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 Pro
You may want to reference Section 3.7 (Pages 80-87) while completing this problem. Using the values for the heat of fusion, specific heat of water, and/or heat of vaporization, calculate the amount of heat energy in each of the following. Keep in mind that the sign of the heat involved in the state change is ignored. 3 E D C R F 5 T ▬▬▬ B FO 6 Q Search H ▼ Part A FZ ▼ N Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us | n 7 Calculate the joules released when 145 g of steam condenses at 100 °C and the liquid cools to 35.0 °C. Express your answer to three significant figures and include the appropriate units. Value Submit Part B ASUS U HA J * 8 Calculate the kilocalories needed to melt a 725 g ice sculpture at 0 °C and to warm the liquid to 35.0 °C. P Pearson M Request Answer F9 1 ( → C a Units K 9 F10 Alt NYE 1 L ? F11 O IA E P : F12 Ctrl - Review | Constants Periodic Table Prt Sc I + 19 = "1 Insert 4x D Delete…
Calculate 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.
Ethanol (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 kJ
Under normal atmospheric pressure, nitrogen boils (and condenses) at -196oC. When 7.7 g of nitrogen gas at -196oC was put into a dewar flask initially at -260oC, their temperatures reach -210oC. The specific heat capacity and heat of vaporization of nitrogen are 1.04 J/g-oC and 200 J/g. Based on the system described above, is the following statement true or false? The nitrogen released heat and the flask absorbed it.
A 25.5-g sample of ice at -10.0°C is mixed with 110.0 g water at 85.0°C. Calculate the final temperature (in °C) of the mixture assuming no heat loss to the surroundings. The heat capacities for H₂O(l) and H₂O(s) are 4.184 J/g･°C and 2.03 J/g･°C, respectively, and the enthalpy of fusion of ice is 6.02 kJ/mol.