The following information is given for cobalt at latm:AHvap(3097 °C) = 389kJ/molboiling point = 3097 °CAHfus(1495 °C) = 15.5kJ/molmelting point = 1495 °Cspecific heat solid= 0.418 J/g°C_specific heat liquid = 0.686Jig°CWhat is AH in kJ for the process of freezing a 22.9 g sampleof liquid cobalt at its normal melting point of 1495 °C.kJSubmit AnswerRetry Entire Group

The heat capacity is the ratio of the energy supplied in the form of heat to the rise in the…

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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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Use the References to access important values if needed for this question. The following information is given for antimony at 1 atm: T = 1440.00°C AHvap (1440.00°C) = 1.605 x 10 J/g %3D Tm = 631.00°C AHfus (631.00°C) = 161.1 J/g Specific heat solid 0.2090 J/g °C Specific heat liquid = 0.2590 J/g °C A 35.20 g sample of solid antimony is initially at 613.00°C. If the sample is heated at constant pressure (P = 1 atm), kJ of heat are needed to raise the temperature of the sample to 827.00°C.
The heat of formation of liquid methoxyethane (CH₂OC₂H₂) is -216.4 kJ/mol. Which of the following is the correct heat of formation reaction for liquid methoxyethane? A. O B. O C. O D. O E. O 6 C(s, graphite) + 8 H₂(g) + O2(g) → 2 CH3OC2H5 (1) 6 CO₂ (s) + 8 H₂O(g) → 2 CH3OC₂H5(1) + 9 O₂(g) 3 C(s, graphite) + 4 H₂(g) + C₂(3, graphite) + 4 H₂(g) + O2(g) → CH3OC₂H5 (1) O₂(g) → CH3OC2H5(1) 3 C(s, graphite) + 8 H(g) + O(g) → CH3OC₂H5 (1) kJ ΔΗ = -216.4 mol ΔΗ; = -216.4 ΔΗ ΔΗ ΔΗ == -216.4 kJ mol = -216.4 -216.4 == kJ mol kJ mol kJ mol
Use the References to access important values if needed for this question. The following information is given for manganese at 1 atm: ДHap (2095.00°C) — 4.090 х 10° J/g AĦfus (1244.00°C) = 266.5 J/g Ть 3 2095.00°С Tm = 1244.00°C Specific heat solid = 0.4770 J/g °C Specific heat liquid = 0.8370 J/g °C A 28.60 g sample of solid manganese is initially at 1222.00°C. If the sample is heated at constant pressure (P = 1 atm), kJ of heat are needed to raise the temperature of the sample to 1383.00°C.
The following information is given for lead at 1 atm: AHrap (1740.00°C) = 858.2 J/g AHfus (328.00°C) = 23.00 J/g %3D ТЬ 3 1740.00°C Tm = 328.00°C Specific heat solid = 0.1300 J/g °C Specific heat liquid J/g °C %3D 0.1380 %3D A 23.40 g sample of solid lead is initially at 310.00°C. If the sample is heated at constant pressure (P = 1 atm), kJ of heat are needed to raise the temperature of the sample to 575.00°C.
What quantity of heat (in kJ) will be absorbed by a 82.3 g piece of aluminum (specific heat = 0.930 J/g･ °C) as it changes temperature from 23.0 °C to 67.0 °C?
How much heat, in joules and in calories, must be added to a 89.9 g manganese block with a specific heat of 0.479 J/g·°C to increase its temperature from 25°C to its melting temperature of 1246°C? Answer in J and in cal
A 5.34g sample of aluminum at 23oC absorbs 170 J of heat. What is the new temperature of the sample? CAl = 0.900 J/goC
The following information is given for lead at 1atm: AHvap (1740.00°C) = 858.2 J/g AHfus (328.00°C) = 23.00 J/g T = 1740.00°C Tm = 328.00°C Specific heat solid = 0.1300 J/g °C Specific heat liquid = 0.1380 J/g °C %3D A 39.80 g sample of liquid lead at 478.00°C is poured into a mold and allowed to cool to 23.00°C. How many kJ of energy are released in this process? (Report the answer as a positive number.) Energy = kJ
References Use the References to access important values if needed for this question. The following information is given for magnesium at 1 atm: AHvap (1090.00°C) = 5.424 x 10° J/g AHfus (649.00°C) = 368.3 J/g T = 1090.00°C Tm = 649.00°C Specific heat solid = 1.017 J/g °C Specific heat liquid = 1.339 J/g °C A 34.00 g sample of solid magnesium is initially at 619.00°C. If the sample is heated at constant pressure (P= 1 atm), kJ of heat are needed to raise the temperature of the sample to 768.00°C. Submit Answer
Oo.153. Subj :- Chemistry
Find the total energy involved in converting 450.0g of water from -21°C to 35°C. Hvan Water = 40.7 KJ/mol Hrus Water = 6.01 KJ/mol Solid C =2.03 J/g°C water Liquid Cwater =4.184 J/g°C Gas Cwater 2.01 J/g°C O 235 KJ O 150 KJ O 85 KJ 255 KJ
5

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