The following information is given for mercury at latm: AHvap(357°C)= 59.3 kJ/mol boiling point 357 °C AHfus(-39 °C)= 2.33 melting point -39 °C kJ/mol specific heat solid= 0.141 J/goC specific heat liquid J/g°C 0.139 What is AH in kJ for the process of freezing a 49.0 g sample of liquid mercury at its normal melting point of -39 °C

The following information is given for mercury at latm: AHvap(357°C)= 59.3 kJ/mol boiling point 357 °C AHfus(-39 °C)= 2.33 melting point -39 °C kJ/mol specific heat solid= 0.141 J/goC specific heat liquid J/g°C 0.139 What is AH in kJ for the process of freezing a 49.0 g sample of liquid mercury at its normal melting point of -39 °C

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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Calculate the total energy (kJ) required to heat a 17.5 g sample of benzene (C6H6) from 0 °C to 97.2 °C molar mass: 78.11 g/mol cs,solid = 1.51 J/g*°C cs,liquid = 1.70 J/g*°C cs,gas = 1.05 J/g*°C ΔHfus = 9.9 kJ/mol ΔHvap = 33.8 kJ/mol Tf = 5.6°C Tb = 80.08°C
The following questions refer to the reaction below. N2(g) + O2(g) 2 NO(g) AH° = 181.8 kJ 1. This reaction is Oexothermic Oendothermic 2. Heat is Oreleased Oabsorbed by the chemicals in this reaction. 3. Calculate AH° for the reaction YouTube 4 NO(g) 2 N2(g) + 2 O2(g) AH° = kJ 4. Calculate the standard heat of formation of NO. AH°t kJ %3D 5. Calculate the amount of heat transferred when 3.000 g of N2 are reacted with excess O2 gas.
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.
26. From the following information, determine AS° for the following: N(g) + O(g) NO(g) AS°=? > N2(g) + O2(g) → 2NO(g) AS°=24.8 J/K N2(g) 2N(g) AS°=115.0 J/K O2(g) 20(g) AS°=117.0 J/K
THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the hypothetical reaction: (Round off the final answer to ONE decimal place. Do not include the unit.) 2X2D (g) + 3M2 (g) – 2X2M (I) + 2DM2 (g) AH°f for X2D (g) = -26 kJ/mol AH°f for DM2 (g) = -296.8 kJ/mol AH°f for X2M (1) = -286.5 kJ/mol AH°f for M2 (g) = 0 kJ/mol
Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction: 2Al(s) + Fe203(s) → Al203(s) + 2Fe(s) This reaction occurs when a mixture of powdered aluminum and iron(III) oxide is ignited with a magnesium fuse. The following enthalpies of formation are known: AH°; for Fe203(s) = -826 kJ AH°; for Al203(s) = -1676 kJ O 1251 kJ O 2502 kJ O-1251 kJ O 425 kJ 850 kJ O- 2502 kJ -850 kJ -425 kJ
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?
The addition of 105.0 g potassium fluoride to 599.0 mL of water (d = 1.00 g/mL) causes the temperature to rise 3.21 °C. What is the ΔHrxn for KF? (Assume cp = 4.18 J/g oC.)
Using the following thermochemical data: 2Er(s) + 6HF(g) → 2ErF3(s) + 3H2(g) ΔH° = -1795.4 kJ/mol 2Er(s) + 6HCl(g) → 2ErCl3(s) + 3H2(g) ΔH° = -1443.6 kJ/mol calculate ΔH° for the following reaction:ErF3(s) + 3HCl(g) → ErCl3(s) + 3HF(g) 351.8 kJ/mol -3239.0 kJ/mol -1619.5 kJ/mol 703.6 kJ/mol 175.9 kJ/mol
Butane, C4H10, is vaporized at its boiling point. C4H10(1) → C4H10(g) AH° = 301.5 kJ/mol, ASº = 761.4 J/mol·K Calculate the boiling point temperature (in K) at standard conditions.