Use the References to access important values if needed for this question.The following information is given for lead at 1 atm:boiling point = 1740 °Cmelting point = 328 °CAHvap(1740 °C) = 177.8 kJ/molAHfus (328 °C) = 4.77 kJ/molspecific heat solid = 0.130 J/g°Cspecific heat liquid=0.138 J/g°CWhat is AH in kJ for the process of freezing a 39.5 g sample of liquid lead at its normalmelting point of 328 °C?kj

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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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the laboratory a student finds that it takes 101 Joules to increase the temperature of 13.6 grams of solid iodine from 20.6 to 39.3 degrees Celsius. e specific heat of iodine calculated from her data is J/g°C.
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A 125 g piece of rock of unknown specific heat is heated to 93 degrees C. The rock is then dropped into 100 g of water at 19 degrees C. the water temperature rises to 31 degrees C. What is the specific heat of the rock? (3) O 0.65 J/(g °C) O 0.65 J O 0.71 J/g °C) O 1.14 J/g.
The lattice energy is defined as the energy required to break one mole of an ionic solid into its ions in the gas phase. The lattice energy for calcium oxide corresponds to the following reaction. CaO(s) Ca2+(g) + O2-(g) DH = ? Using the following information, determine the lattice energy for calcium oxide. Ca(s) ----> Ca(g) DH = 178.2 kJ Ca(g) ----> Ca2+(g) + 2e- DH = 1747.9 kJ O2(g) ----> 2O(g) DH = 498.3 kJ O2-(g) ----> O(g) + 2e- DH = -702 kJ Ca(s) + 1⁄2 O2(g) ----> CaO(s) DH = -635.0 kJ Using the unrounded answer from the previous problem determine q (kJ) for the following reaction when 1.00 grams of solid calcium oxide forms. Ca2+(g) + O2-(g) ⟶⟶ CaO(s)
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IT The temperature of a sample of aluminum increased by 24.6 °C when 255 J of heat was applied. Substance Specific heat J/(g lead 0.128 What is the mass of the sample? silver 0.235 copper 0.385 iron 0.449 aluminum 0.903 m =
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How many grams of an unknown substance, having a specific heat of 1.66 J g ° C, are present if a temperature change of -173.4 K occurs. The heat lost was 35981 J.
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
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