The following information is given for antimony at 1atm:Th = 1440.00°CΔΗ,vap (1440.00°C) = 1.605 x 10³ J/gTm = 631.00°CSpecific heat solid = 0.2090 J/g °CSpecific heat liquid = 0.2590 J/g °CAHfus (631.00°C) = 161.1 J/gA 40.40 g sample of liquid antimony at 721.00°C is poured into a mold and allowed to cool to 25.00°C. How many kJ of energy are released in this process?(Report the answer as a positive number.)Energy =kJ

Answered: Image /qna-images/answer/4298709f-29df-455e-ad62-ed7d671071e5.jpg

The following information is given for antimony at 1atm: AHvap (1440.00°C) = 1.605 ×x 10° 1/g AĦfus (631.00°C) = 161.1 J/g T, = 1440.00°C Tm = 631.00°C Specific heat solid = 0.2090 J/g °C Specific heat liquid = 0.2590 J/g °C A 40.40 g sample of liquid antimony at 721.00°C is poured into a mold and allowed to cool to 25.00°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 antimony at 1atm: AHvap (1440.00°C) = 1.605 ×x 10° 1/g AĦfus (631.00°C) = 161.1 J/g T, = 1440.00°C Tm = 631.00°C Specific heat solid = 0.2090 J/g °C Specific heat liquid = 0.2590 J/g °C A 40.40 g sample of liquid antimony at 721.00°C is poured into a mold and allowed to cool to 25.00°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...

See similar textbooks

Similar questions

The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. What is qH2O?
Given the following thermochemical equations P4(s) + 6C12(g) 4PCI3(g) AH = -2439 kJ/mol 4PCI5(g) → P4(s) + 10CI 2(g) AH = 3438 kJ/mol find the AH for the reaction below, PCI5(g) → PC|3(g) + Cl2(g) O A) +249.8 kJ/mol O B) +999 kJ/mol O C) -999 kJ/mol O D) -249.8 kJ/mol
2 NO(g) N2(g) + O2(g) H = -180.7 kJ 2 NO(g) + O2(g) 2 NO2(g) H = -113.1 kJ 2 N2O(g) 2 N2(g) + O2(g) H = -163.2 kJ Use Hess's law to calculate H for the reaction below.3 NO(g) N2O(g) + NO2(g)H = _____k J
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
Oo.153. Subj :- Chemistry
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.
A container of water is heated with 10 J of energy at constant pressure. What is the enthalpy change (AH) for this process? O >10 J +10 J -10 J O <10 J O O J
Which substance will have the largest temperature change if the same amount of heat is added to each of them?Gold, Au(s): specific heat = 0.0308 calories per gram degree Celsius.Water, H2O(l): specific heat = 1.00 calorie per gram degree Celsius.Copper, Cu(s): specific heat = 0.0920 calorie per gram degree Celsius.Ethanol, C2H5OH(l): specific heat = 0.588 calorie per gram degree Celsius
The following information is given for silver at 1 atm: AHvap (2212.00°C) = 2.355 x 10° J/g AĦtus (961.00°C) = 110.8 J/g T, = 2212.00°C Tm = 961.00°C Specific heat solid = 0.2380 J/g °C Specific heat liquid = 0.2850 J/g °C A 39.00 g sample of solid silver is initially at 938.00°C. If the sample is heated at constant pressure (P=1 atm), temperature of the sample to 1263.00°C. kJ of heat are needed to raise the
Given these reactions, where X represents a generic metal or metalloid 1) H2(g)+12O2(g)⟶H2O(g)Δ?1=−241.8 kJ1) H2(g)+12O2(g)⟶H2O(g)ΔH1=−241.8 kJ 2) X(s)+2Cl2(g)⟶XCl4(s)Δ?2=+159.7 kJ2) X(s)+2Cl2(g)⟶XCl4(s)ΔH2=+159.7 kJ 3) 12H2(g)+12Cl2(g)⟶HCl(g)Δ?3=−92.3 kJ3) 12H2(g)+12Cl2(g)⟶HCl(g)ΔH3=−92.3 kJ 4) X(s)+O2(g)⟶XO2(s)Δ?4=−517.9 kJ4) X(s)+O2(g)⟶XO2(s)ΔH4=−517.9 kJ 5) H2O(g)⟶H2O(l)Δ?5=−44.0 kJ5) H2O(g)⟶H2O(l)ΔH5=−44.0 kJ what is the enthalpy, Δ?,ΔH, for this reaction? XCl4(s)+2H2O(l)⟶XO2(s)+4HCl(g)
The following information is given for diethyl ether at 1 atm: AHvap (34.60°C) = 357.5 J/g AHtus (–116.30°C) = 98.10 J/g T = 34.60°C Tm =-116.30°C Specific heat gas = 1.460 J/g °C Specific heat liquid = 2.320 J/g °C A 25.20 g sample of liquid diethyl ether is initially at -4.30°C. If the sample is heated at constant pressure (P = 1 atm), kJ of energy are needed to raise the temperature of the sample to 53.40°C.
The combustion of 1.925 g of propanol (C₂H,OH) increases the temperature of a bomb calorimeter from 298.00 K to 302.14 K. The heat capacity of the bomb calorimeter is 15.61 kJ/K. Determine AH for the combustion of propanol to carbon dioxide gas and liquid water. kJ/mol ΔΗ = TOOLS x10