5.9) How much energy would be required to vaporize (boil) 50.0 grams of each of the following substances? a) water ANSWER: 27000 cal (two significant figures) b) ethanol ANSWER: 12000 cal (two significant figures) c) 2-propanol ANSWER: 7950 cal (three significant figures) Substance H₂O ethanol (ethyl alcohol) 2-propanol (rubbing alcohol) heat of fusion (Hfus) 79.7 cal/g 26.05 cal/g 21.37 cal/g heat of vaporization (Hvap) 540 cal/g 230 cal/g 159 cal/g

5.9) How much energy would be required to vaporize (boil) 50.0 grams of each of the following substances? a) water ANSWER: 27000 cal (two significant figures) b) ethanol ANSWER: 12000 cal (two significant figures) c) 2-propanol ANSWER: 7950 cal (three significant figures) Substance H₂O ethanol (ethyl alcohol) 2-propanol (rubbing alcohol) heat of fusion (Hfus) 79.7 cal/g 26.05 cal/g 21.37 cal/g heat of vaporization (Hvap) 540 cal/g 230 cal/g 159 cal/g

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter5: Gases, Liquids, And Solids

Section: Chapter Questions

Problem 5.74P

See similar textbooks

Similar questions

7:36 How many moles of C4H₁0 (isobutane) must be reacted according to the following balanced chemical reaction to transfer -187.5 KJ of heat? 2 C4H10(g) + 13 O₂(g) → H₂O(g) ΔΗ = -2868.8 STARTING AMOUNT ADD FACTOR x( ) 13 15.30 2 Question 21 of 25 0.1307 10 5.379 x 105 -187.5 7.650 6.022 x 10²3 1 4 5 X 8 8 ANSWER 9 KJ 0.06536 -2868.8 Submit Tap here or pull up for additional resources CO₂(g) + 10 RESET 5 g CO₂ g C4H₁0 mol CO₂ g 0₂ kJ mol C4H10 g mc mol
(Q46) How much heat (in kJ) is released when 32.2 grams of liquid bromine (Br2) is cooled from an initial temperature of 7.3°C to a final temperature of -16.9 °C? (3 sf) Cs liquid = 0.4737 J/g.°C %3D Cs gas = 0.2262 J/g.°C Melting point = -7.19°C %3D AHfusion = 10.52 kJ/mol
How many grams of water can be heated from 28.3°C to 41.8°C by the heat released from 83.5 g of lead that cools from 77.6°C to 28.9°C? i g H20(1) eTextbook and Media Attempts: 0 of 15 used Submit Answer Save for Later OCT étv 25 МacBook Air DII DD F10 888 F4 F9 FB F7 F5 F3 F2
A coffee-cup calorimeter contains 50 of water with an initial temperature of 24.8 degrees * C . An unknown sample with a mass of 1.972 grams was placed inside making the water temperature rise up to 25.5 degrees * C The initial temperature of the metal was 98.3C 1. What is the specific heat (J/g C) of the unknown sample? round off final answer to 2 decimal places
A certain coal has the following ultimate analysis C=70%, N2=4%, H2=2.5%, O2=3.5%, S2=7%, Ash=5%, Moisture=2% Determine the heating value of fuel in Btu/lb. ANSWER: 11,735.351
KINETIC ENERGY (3) 10 9 T Select the graph that shows the correct relationship between kinetic energy and mass. Hint: If one object has 2 times the mass of a second object and their speeds are the same, then the first object has 2 times the kinetic energy of the second object. KINETIC ENERGY (1) g**** MASS (kg) 10 S 2 Zeam Math: A Pers Desk 2 15 M KINETIC ENERGY (J) KINETIC ENERGY (3) 10 10 Run 3-Unblocked G E MASS (kg) YouTube 10 15 I : C
RESULTS Make sure to use correct significant figures and units of measure. HOT WATER/COOL WATER temperature change for hot water:_ temperature change for cool water: 50(-37(= 378 -20°c =178 (4.18 (50.0g) (378_50, heat leaving hot water: 2717 J heat absorbed by cool water: 35533 (4.18)) (150.08) (37°C-20)=3553J heat capacity of calorimeter: 49.12 HCI/NaOH HC₂H302/NH3 13.c (2717J-35535) = 49.17 J 17°C (400-200)= change of temperature: ⁰°C heat emitted during reaction: heat of neutralization, AH₁: FIVE STAR. ***** 50,0)
The heating curve shown was generated by measuring the heat flux and temperature for a solid that was heated. The slope of the segment CD, corresponds to the heat capacity of the liquid of the substance. Select one:RealFalse
1:13 0 * ll 66%i Cyra Garces Active Now CALORIMETRY HEAT OF FUSION Trial 1 Trial 2 Mass of ice M (grams) 79 79 Mass of warm water Mter (grams) 120 119 Initial temperature of water Tinitial ("C) 41 42 Final temperature of mixture Tfinal ("C) -4 Calculated heat of fusion of ice Leperinemtal (cal/g) 72.4 60.8 Standard value of heat of fusion of ice Lemdard (cal/g) 79.7 79.7 Percentage error 9.22% 23.76% Calculations According to the principle of the conservation of energy, the quantity of heat absorbed by the ice as it melts (Quained melring) and then heats up to the final equilibrium temperature (Qpain by melted ice) must equal the quantity of heat released by the warm water (Qlast by warm water) as it cools down to the final equilibrium temperature. Mathematically: le guined metingl iast by warm water pained meltingl + o cat (M(L) + (M)(1)T - OC) = (Mt(1)(Tie- T fina - 0C) - (Mt(1 final water initial More Edit II -
What is the amount of heat (in Joules) required to completely boil away 2000 grams of room temperature (23 °C) water?
2,3,4
Octane (C8H18) is a chemical compound in gasoline. When gasoline burns, the octane reacts with oxygen to produce carbon dioxide, water and 5471 kJ of heat 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O + 5471 kJ If you want to obtain 12.5 kJ of heat by reacting octane with oxygen, how many grams of octane must you use? a.)0.109 g b.)0.522 g c.)25.0 g d.)438 g