A mass of 31.5 g of H20(g) at 373 K is allowed to flow into 279 g of H20(1) at 298 K and 1 atmPart ACalculate the final temperature of the system once equilibrium has been reached. Assume that Cp m for H,O is constant at its values for 298 K (75.3 J. mol1.K 1) throughout the temperature range of interest AHyan for water is 40650J. mol 1Express the temperature in kelvins to three significant figures.T = KSubmitRequest Answer

In case of mixing of two liquids at different temperature, the final temperature of final solution…

A mass of 31.5 g of H20(g) at 373 Kis allowed to flow into 279 g of H2O(1) at 298 K and 1 atm Part A Cem for H,O is constant at its values for 298 K (75.3 J. mol 1. K 1) throughout the temperature range of interest AHan for water is 40650 Calculate the final temperature of the system once equilibrium has been reached. Assume J. mol 1 Express the temperature in kelvins to three significant figures. T = K Submit Reguest Answer

A mass of 31.5 g of H20(g) at 373 Kis allowed to flow into 279 g of H2O(1) at 298 K and 1 atm Part A Cem for H,O is constant at its values for 298 K (75.3 J. mol 1. K 1) throughout the temperature range of interest AHan for water is 40650 Calculate the final temperature of the system once equilibrium has been reached. Assume J. mol 1 Express the temperature in kelvins to three significant figures. T = K Submit Reguest Answer

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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33.6 g of a salt solution was mixed with 27.5 g of water in a calorimeter with a calorimeter constant of 66.5 J K-1 with all substances initially at 30.9 °C. The resulting solution was observed to be at a temperature of 12.2 °C and have a heat capacity of 3.97 J g K-1. Determine q for the mixing process. Oa. -5780 J Ob. 4540 J Oc. 8.05 x 104 J Od. 5780 J Oe. -7.86 x 104 J
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00 Turkcell 3G 03:22 @ %27D 3. When 120 mg of naphthalene, CH, (s), was burned in a bomb calorimeter the temperature rose by 3.05 K a) Calculate the calorimeter constant. b) By how much will the temperature rise when 10 mg of phenol, C,HOH(s), is bumed in the calorimeter under the same conditions? (AH n.- -5156.3 kJ/mol and Mw CH 128.17 g/mol, AH° CESON = -3054 kJ/mol, Mw CO94.12 g/mol) 4 At 25°C, the density of a 50 % by mass ethanol/water solution is 0.914 g cm. Given that the partial molar volume of water in this solution is 17.4 cm'mol'. What is the partial molar volume of the ethanol? (d 0.789 g/cm': d-1.00 g cm": Mw for water-18 g mot', ethanol-46.07g mot 5. The addition of 5.00 g of a compound to 250 g of naphthalene lowered the freezing point of naphthalene by 0.780 K. Calculate the molar mass of the compound. (K, 694 KAgmol for naphthalene)
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A 84.8-g piece of silver (s = 0.237 J/(g. °C)), initially at 268.0°C, is added to 128.4 g of a liquid, initially at 24.9°C, in an insulated container. The final temperature of the metal-Hiquid mixture at .equilibrium is 39.6°C. What is the identity of the liquid? Neglect the heat capacity of the container methanol (s = 2.53 J/(g. °C) .a acetone (s = 2.15 J/(g. °C)) .b 4.18 J/(g. °C)) .c hexane (s = 2.27 J/(g. C)).d water (s = ethanol (s = 2.43 J/(g. °C)) .e
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