The following information is given for bismuth at latm: T = 1627.00°C AHvap (1627.00°C) = 822.9 J/g AHfus (271.00°C) = 52.60 J/g Tm = 271.00°C Specific heat solid = 0.1260 J/g °C Specific heat liquid = 0.1510 J/g °C A 47.10 g sample of liquid bismuth at 503.00°C is poured into a mold and allowed to cool to 30.00°C. How many kJ of energy are released in this process? (Report the answer as a positive number.) Energy = | kJ

The following information is given for bismuth at latm: T = 1627.00°C AHvap (1627.00°C) = 822.9 J/g AHfus (271.00°C) = 52.60 J/g Tm = 271.00°C Specific heat solid = 0.1260 J/g °C Specific heat liquid = 0.1510 J/g °C A 47.10 g sample of liquid bismuth at 503.00°C is poured into a mold and allowed to cool to 30.00°C. How many kJ of energy are released in this process? (Report the answer as a positive number.) Energy = | kJ

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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What is the identity of a 10.0 solid metal sample that has its temperature increased by 14.0°C when q = 53.9 J of heat energy was absorbed? Metal sample: Au: 0.128 Ag: 0.235 Cu: 0.385 Fe: 0.449 Al: 0.903
A 13 g chunk of metal is heated up in a Bunsen burner flame and dropped into an insulated vessel containing 192 g of water at 21.7°C. The final temperature of the system is 25.5°C. What is the initial temp of the metal? (Assume that no heat is lost to the environment and that no water is lost through vaporization.) Smetal = 0.72 J/g .°C
References Use the References to access important values if needed for this question. The following information is given for iron at 1 atm: = 2750.00°C AHvap (2750.00°C) = 6.338 x 10° J/g AĦfus ( 1535.00°C)= 289.2 J/g Tm =1535.00°C %3D Specific heat solid = 0.4520 J/g °C Specific heat liquid = 0.8240 J/g °C %3D A 42.10 g sample of solid iron is initially at 1511.00°C. If1.869 × 10* J of heat are added to the sample at constant pressure (P = 1 atm), which of the following is/are true? (Select all that apply.) O The sample is a liquid. OThe sample is a gas. The sample is a solid in equilibrium with liquid. The sample is at a temperature greater than 1535.00°C. The sample is at a temperature of 1535.00°C. Submit Answer
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An insulated container is used to hold 46.8 g of water at 25.8 °C. A sample of copper weighing 14.5 g is placed in a dry test tube and heated for 30 minutes in a boiling water bath at 100.0°C. The heated test tube is carefully removed from the water bath with laboratory tongs and inclined so that the copper slides into the water in the insulated container. Given that the specific heat of solid copper is 0.385 J/(g·°C), calculate the maximum temperature of the water in the insulated container after the copper metal is added. °C
The following information is given for silicon at 1 atm: (2355.00°C) =1.058 × 10ª J/g AHvap = 2355.00°C Tm = 1410.00°C AĦUS (1410.00°C) = 1.653 × 10° J/g Specific heat solid = 0.7110 J/g °C Specific heat liquid = 0.9080 J/g °C A 25.40 g sample of solid silicon is initially at 1391.00°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 1674.00°C.
An insulated container is used to hold 41.0 g of water at 22.6 °C. A sample of copper weighing 9.20 g is placed in a dry test tube and heated for 30 minutes in a boiling water bath at 100.0°C. The heated test tube is carefully removed from the water bath with laboratory tongs and inclined so that the copper slides into the water in the insulated container. Given that the specific heat of solid copper is 0.385 J/(g·°C), calculate the maximum temperature of the water in the insulated container after the copper metal is added.
12. An 1855 grams sample of water, initially at 28.6°C, was heated under a pressure of 760 Torr to obtain the same mass of water at 166.0°C. The following data is available for C =2.10 J/g°C Cmam = 2.00 J/g°C water: Allsion=6.02 KJ/mole AHup Cwnur = 4.18 J/g°C %3D = 40.7 KJ/mole (a) Draw the temperature profile for the above process in the space provided below. (b) Calculate the total amount of heat, in kilojoules, required for the above process. (c) What is the energy in Kilocalories and is it exothermic, endothermic; or adiabatic?
How much energy, in units of J, is required to heat 67.5 g of solid acetone from -145.3°C to -101.0°C? The following information may be useful: AfusH = 7.27 kJ mol-1 Cliq = 2.16 J gʻ1 °C-1 %3D Cgas = 1.29 J g-1 °c-1 Csol = 1.65 J g-1 °C-1 Tmelting = -95.0 °C %3D
The following information is given for bismuth at 1 atm: Tb 1627.00°C AHvap (1627.00°C) = 822.9 J/g = Tm = 271.00°C AHfus (271.00°C) = 52.60 3/g Specific heat solid = 0.1260 J/g °C Specific heat liquid = 0.1510 J/g °C A 46.90 g sample of solid bismuth is initially at 253.00°C. If 3.332 x 10³ J of heat are added to the sample at constant pressure ( P = 1 atm), which of the following is/are true? (Select all that apply.) The sample is a gas. The sample is at a temperature of 271.00°C. The sample is at a temperature greater than 271.00°C. The sample is a liquid. The sample is a solid in equilibrium with liquid.
An insulated container is used to hold 41.6 g of water at 22.8 °C. A sample of copper weighing 9.00 g is placed in a dry test tube and heated for 30 minutes in a boiling water bath at 100.0°C. The heated test tube is carefully removed from the water bath with laboratory tongs and inclined so that the copper slides into the water in the insulated container. Given that the specific heat of solid copper is 0.385 J/(g·°C), calculate the maximum temperature of the water in the insulated container after the copper metal is added.
A (4.1700x10^1) g sample of water (C = 4.18 J / g ºC) initially is at (5.110x10^1)ºC. What is the final temperature of this water in ºC if it loses (3.39x10^3) J of heat?