POST EXPERIMENTAL QUESTIONS. and a cooling curve for 1. From your dala, construct a heating curve for ice and a lauric acid by plotting temperature vs time graph Data For Ice metting Tinne (s) Temperature 810 71 73* 0 30 60 1355 8840 870 * 900 76 77 * 930 78 90 120 Сл 5 960 81 * 990 83 6 150 180 16 1020 85 * 1050 86 8 210 1080 87 12 K 240 1110 88 17 270 1140 90* 300 24 * 1170 90 29 330 1200 90 360 33 * 390 35 1230 92 420 37 1260 92* K 450 41 1290 92 92 * 480 411 * 1320 45 1350 93 510 * 48 1380 93 540 1410 93 51 570 1440 93 * 600 54 * 56 1470 94 630 660 59 * 1500 94 * 95 1530 690 60 96 * 1560 720 64 K 750 66 1590 96 96 1620 780 68 I 1650 96 1680 96

POST EXPERIMENTAL QUESTIONS. and a cooling curve for 1. From your dala, construct a heating curve for ice and a lauric acid by plotting temperature vs time graph Data For Ice metting Tinne (s) Temperature 810 71 73* 0 30 60 1355 8840 870 * 900 76 77 * 930 78 90 120 Сл 5 960 81 * 990 83 6 150 180 16 1020 85 * 1050 86 8 210 1080 87 12 K 240 1110 88 17 270 1140 90* 300 24 * 1170 90 29 330 1200 90 360 33 * 390 35 1230 92 420 37 1260 92* K 450 41 1290 92 92 * 480 411 * 1320 45 1350 93 510 * 48 1380 93 540 1410 93 51 570 1440 93 * 600 54 * 56 1470 94 630 660 59 * 1500 94 * 95 1530 690 60 96 * 1560 720 64 K 750 66 1590 96 96 1620 780 68 I 1650 96 1680 96

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...

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Similar questions

The temperature on a sample of pure X held at 1.13 atm and -9. °C is increased until the sample boils. The temperature is then held constant and the pressure is decreased by 0.39 atm. On the phase diagram below draw a path that shows this set of changes. 200 400 temperature (K) pressure (atm)
4. Calculate the amount of energy absorbed when 5g ice @ 0°C melts to water at 0°C. Did a phase change occur? If so, which one? Is this endothermic or exothermic?
An 8.7- g ice cube is placed into 275 g of water. Calculate the temperature change in the water upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from the water and that the ice cube has a temperature of 0 ∘C .
How much heat energy, in kilojoules, is required to convert 51.0 g of ice at –18.0 °C to water at 25.0 °C ? Express your answer to three significant figures and include the appropriate units.
4. How much heat, in kJ, does it take to heat 10.0 g of ice from -24.0°C to 75.0°C? 5. Calculate the amount of heat, in kilojoules, required to convert 180 grams of water at 10.0°C to steam at 105.0 °C. How much heat would be released in the reverse process?
How much heat is needed to convert 936. g of ice at 10.0 °C to steam at 126.0 °C? Be sure your answer has the correct number of significant digits. Note: Reference the Phase change properties of pure substances table for additional information. Water phase Specific heat Solid Liquid Gas kJ 2.03 4.184 1.99 x10 J g.°C J g.°C J g.°℃
Calculate number of joules of energy needed to convert 18 g of ice at -5.0 degrees celsius to liquid water at 75 degrees celsius. Specific Heats: Ice: 2.10 J/g*C Water: 4.184 J/g*C Steam: 2.03 J/g*C Physical Changes: Heat Fusion: 6.02 kj/mol Heat Vapor: 40.8 kj/mol
4. How much energy does it take to convert 75.0 g of ice at -30.0°C to water at 0.0°C?