Foundations of College Chemistry 15e Binder Ready Version + WileyPLUS Registration Card
15th Edition
ISBN: 9781119231318
Author: Morris Hein
Publisher: Wiley (WileyPLUS Products)
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Chapter 13, Problem 34AE
Interpretation Introduction
Interpretation:
Whether liquid water at
Concept Introduction:
Heat of vaporization is the quantity of heat absorbed on vaporization of a liquid. Every substance has different heat of vaporization. It is represented as
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Students have asked these similar questions
Based on the actual value for AHvap of water, how many kJ of energy are needed to convert 5.00
kg of water into steam at 100 °C?
2.
Please don't provide handwritten solution...
Calculate the heat, in kJ, exchanged in the conversion of 20.0 g of steam at 104 °C to water at
10.5 °C.
J
Specific heat capacity, H20(s) = 2.087
g-ºC
J
Specific heat capacity, H20(1) = 4.184
g.ºC
J
Specific heat capacity, H20(g) = 2.042
g.°C
%3D
AH fus = 6.01 kJ/mol
AH vap
= 40.7 kJ/mol
Chapter 13 Solutions
Foundations of College Chemistry 15e Binder Ready Version + WileyPLUS Registration Card
Ch. 13.2 - Prob. 13.1PCh. 13.2 - Prob. 13.2PCh. 13.3 - Prob. 13.3PCh. 13.3 - Prob. 13.4PCh. 13.4 - Prob. 13.5PCh. 13.5 - Prob. 13.6PCh. 13.5 - Prob. 13.7PCh. 13.5 - Prob. 13.8PCh. 13.6 - Prob. 13.9PCh. 13.6 - Prob. 13.10P
Ch. 13 - Prob. 1RQCh. 13 - Prob. 2RQCh. 13 - Prob. 3RQCh. 13 - Prob. 4RQCh. 13 - Prob. 5RQCh. 13 - Prob. 6RQCh. 13 - Prob. 7RQCh. 13 - Prob. 8RQCh. 13 - Prob. 9RQCh. 13 - Prob. 10RQCh. 13 - Prob. 11RQCh. 13 - Prob. 12RQCh. 13 - Prob. 13RQCh. 13 - Prob. 14RQCh. 13 - Prob. 15RQCh. 13 - Prob. 16RQCh. 13 - Prob. 17RQCh. 13 - Prob. 19RQCh. 13 - Prob. 20RQCh. 13 - Prob. 21RQCh. 13 - Prob. 22RQCh. 13 - Prob. 23RQCh. 13 - Prob. 24RQCh. 13 - Prob. 25RQCh. 13 - Prob. 26RQCh. 13 - Prob. 27RQCh. 13 - Prob. 28RQCh. 13 - Prob. 29RQCh. 13 - Prob. 30RQCh. 13 - Prob. 31RQCh. 13 - Prob. 32RQCh. 13 - Prob. 33RQCh. 13 - Prob. 34RQCh. 13 - Prob. 35RQCh. 13 - Prob. 36RQCh. 13 - Prob. 37RQCh. 13 - Prob. 38RQCh. 13 - Prob. 39RQCh. 13 - Prob. 40RQCh. 13 - Prob. 41RQCh. 13 - Prob. 42RQCh. 13 - Prob. 43RQCh. 13 - Prob. 1PECh. 13 - Prob. 2PECh. 13 - Prob. 3PECh. 13 - Prob. 4PECh. 13 - Prob. 5PECh. 13 - Prob. 6PECh. 13 - Prob. 7PECh. 13 - Prob. 8PECh. 13 - Prob. 9PECh. 13 - Prob. 10PECh. 13 - Prob. 11PECh. 13 - Prob. 12PECh. 13 - Prob. 13PECh. 13 - Prob. 14PECh. 13 - Prob. 15PECh. 13 - Prob. 16PECh. 13 - Prob. 17PECh. 13 - Prob. 18PECh. 13 - Prob. 19PECh. 13 - Prob. 20PECh. 13 - Prob. 21PECh. 13 - Prob. 22PECh. 13 - Prob. 23PECh. 13 - Prob. 24PECh. 13 - Prob. 25PECh. 13 - Prob. 26PECh. 13 - Prob. 27PECh. 13 - Prob. 28PECh. 13 - Prob. 29PECh. 13 - Prob. 30PECh. 13 - Prob. 31PECh. 13 - Prob. 32PECh. 13 - Prob. 33AECh. 13 - Prob. 34AECh. 13 - Prob. 35AECh. 13 - Prob. 36AECh. 13 - Prob. 38AECh. 13 - Prob. 39AECh. 13 - Prob. 40AECh. 13 - Prob. 41AECh. 13 - Prob. 42AECh. 13 - Prob. 43AECh. 13 - Prob. 44AECh. 13 - Prob. 45AECh. 13 - Prob. 46AECh. 13 - Prob. 47AECh. 13 - Prob. 48AECh. 13 - Prob. 49AECh. 13 - Prob. 50AECh. 13 - Prob. 51AECh. 13 - Prob. 52AECh. 13 - Prob. 53AECh. 13 - Prob. 54AECh. 13 - Prob. 55AECh. 13 - Prob. 56AECh. 13 - Prob. 57AECh. 13 - Prob. 58AECh. 13 - Prob. 59AECh. 13 - Prob. 60AECh. 13 - Prob. 61AECh. 13 - Prob. 62AECh. 13 - Prob. 63AECh. 13 - Prob. 64AECh. 13 - Prob. 65AECh. 13 - Prob. 66AECh. 13 - Prob. 67AECh. 13 - Prob. 69CECh. 13 - Prob. 70CECh. 13 - Prob. 71CECh. 13 - Prob. 72CE
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- 12.) A 36.0 g sample of liquid water at 100.0oC is heated to 145.0 oC. How much heat does the water absorb in this process? What is its phase at the end? You will need to use some of the information given below. Specific Heat Capacities: CS(H2O,s) = 2.09 J/g oC; CS(H20, l) = 4.18 J/g oC; CS(H2O,g) = 2.01 J/g oC ΔHofus = 6.02 kJ/mol; ΔHovap = 40.7 kJ/mol.arrow_forward2)What is the definition of boiling point? How is the boiling point affect by atmosphericpressure and why? 2-1) What is the definition of standard state?arrow_forwardSulfur dioxide is produced in enormous amounts for sulfuric acid production. It melts at −73.0°C and boils at −10.0°C. Its ΔHfus is 8.619 kJ/mol, and its ΔHvap is 25.73 kJ/mol. The specific heat capacities of the liquid and gas are 0.995 J/g·K and 0.622 J/g·K, respectively. How much heat is required to convert 5.000 kg of solid SO2 at the melting point to a gas at 60.0 degrees C? Answer should be in J.arrow_forward
- How long would it take for 1.50 molmol of water at 100.0 ∘C∘C to be converted completely into steam if heat were added at a constant rate of 20.0 J/sJ/s ?arrow_forwardIf 30.0 g of steam at 120.0°C is pumped into an insulated vessel containing 400. g of water at 10.0°C, what will be the equilibrium temperature of the mixture? Sp. heat of H2O(l) = 4.18 J/g-°C, Sp. heat of H2O(g) = 2.03 J/g-°C, heat of vap. of H2O(l) = 2.260 kJ/g)arrow_forwardCompound Z has a heat of vaporization of 155.9 J/g, a specific heat capacity of 2.08 J/gºC, and boils at 72.1ºC. How much energy is required to heat 562.4 g of liquid compound Z from 33.1ºC to a gas at 72.1ºC? Give your answer in kJ to 3 sig figs.arrow_forward
- Calculate the quantity of heat required to convert 70.5 g of H2O(s) at -25°C to H2O(g) at 125°C. fusH of ice at 0°C is 333 J g-1 vapH of liquid water at 100°C is 2260 J g-1 Specific heat capacity of H2O(s) = 2.06 J g-1 K -1 Specific heat capacity of H2O(l) = 4.184 J g -1 K -1 Specific heat capacity of H2O(g) = 1.92 J g-1 K -1 answer in KJarrow_forward21) much heat is required to raise the temperature of the sample to 30.0°C? A benzene sample with a mass of 47.7 g is removed from a freezer at an initial temperature of -10.2°C. How (A) (B) (C) (D) (E) 6.06 kJ 476 k) 9.18 kl 3.12 kJ 8.39 k)arrow_forward(a) If 83.0 g of ice at 0.0oC is placed in 235mL of water at 28.0oC, find the final temperature of water when all of the ice melts. DHfus=6.01 kJ/mol and assume for liquid water density= 1.00 g/mL HINT: you have two parts to find the heat.(remember that the heat lost must equal the heat gained). Part a- find the heat for 83 g of ice melting and then the heat for the liquid to warm up Part b- find the heat for 235 mL H2O to cool down (b) What is the interpretation/finding from this problem?arrow_forward
- EVALUATE: 2. The heat of vaporization of water at 1000C is 2.26 kJ/g; at 370C it is 2.41kJ/g. a, What is the standard molar heat of vaporization at 37 C? b. Why is the heat of vaporization greater at 37°C than at 100 ?arrow_forwardExplain why water boils at higher temperature under higher pressure (pure substance saturation temperature depends on pressure). Use knowledge of energy and energy transferring at molecular or atomic level during the phase change of a substance. You do not need to show calculations. • (a) the amount of heat absorbed as 1 kg of saturated liquid water boils at 100°C. (b) the amount of heat released as 1 kg of saturated water vapor condenses. Is a >b, a=b, or aarrow_forwardH2O has a ΔHvap = 40.8 kJ/mol and a ΔHfus = 6.02 kJ/mol. The specific heat capacity of ice is 2.11 J/g•°C, of liquid water is 4.18 J/g•°C and of steam is 2.00 J/g•°C. Calculate the total heat transferred to elevate 250 g of pure water from –42 °C to 127 °C.arrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
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