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 containermethanol (s =2.53 J/(g. °C) .aacetone (s = 2.15 J/(g. °C)) .b4.18 J/(g. °C)) .chexane (s = 2.27 J/(g. C)).dwater (s =ethanol (s = 2.43 J/(g. °C)) .e

Answered: Image /qna-images/answer/f43cb45b-7f70-4b41-adde-d694560edc3d.jpg

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-liquid mixture at .equilibrium is 39.6°C. What is the identity of the liquid? Neglect the heat capacity of the container h methanol (s = 2.53 J/(g. °C)).a acetone (s = 2.15 J/(g. C)) .b %3D water (s = 4.18 J/(g. C)) .c %3D hexane (s = 2.27 J/(g. C)).d %3D ethanol (s = 2.43 J/(g. C)).e %3D autill aziall

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-liquid mixture at .equilibrium is 39.6°C. What is the identity of the liquid? Neglect the heat capacity of the container h methanol (s = 2.53 J/(g. °C)).a acetone (s = 2.15 J/(g. C)) .b %3D water (s = 4.18 J/(g. C)) .c %3D hexane (s = 2.27 J/(g. C)).d %3D ethanol (s = 2.43 J/(g. C)).e %3D autill aziall

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

For the following reaction 2NO2(g) = N204(g) AH° = -58.02 kJ/mol and AS° = -176.6 J/mol·K. What is AG %D for the reaction at 40.0°C when P_NO2 = P_N2O4 = 0.200 atm? Assume AH° and AS° are temperature independent. t: tr kJ/mol
You weighed your empty insulated cup and found that the mass of the cup was 3.6 g. You add some hot water and find that the total mass increases to 26.3 g. You got some ice from the bus tub, and found that it was wet. After drying it carefully, you take the temperature of the hot water in the cup and find that its temperature is 55.9 °C and then add the ice. The temperature of the water dropped, and came to equilibrium at 35.2 °C. At the end of the experiment you re-weigh the cup and find that the mass has increased to 31.7 g. What is your experimental value for the heat of fusion?
Hw.17.
Calculate the amount of heat released (absolute value) when 0.700 kg of liquid ethanol is burned in excess oxygen to make carbon dioxide and liquid water. The enthalpies of formation of the products and reactants are:CO2(g): -393.51 kJ/molH2O(l): -285.83 kJ/molO2(g): 0 kJ/molC2H5OH(l): -276.0 kJ/mol
The thermite reaction, used for welding iron, is the reaction of FegO4 with Al. 8 Al (s) + 3 Fe3O4 (s) > 4 Al203 (s) + 9 Fe (s) AH° = -3350 kJ Because this large amount of heat cannot be rapidly dissipated to the surroundings, the reacting mass may reach temperatures near 3000°C. How much heat (in kJ) is released by the reaction of 16.5 g of Al with 76.7 g of Fe304? Enter your numerical answer in units of kJ.
30 moles of a gas are contained in a 50 L container subjected to 5 atm, if its temperature decreases from 85 ºC to 27 ºC in an isochoric process, known its molar specific heat Cv = 7/2 · R (where R = 8.31 J / mol · K).b) Determine U, H, Q, and W
What will be the final temperature (°C) in of a 20.0 g piece of iron (Cp=25.09 J/(mol K), molar mass = 55.845 %/mol) initially at 25°C, if it is supplied with 9.5 J from a stove? 25°C
8) Kirchhoff's Law Calculate the reaction enthalpy for the following reaction (ARH° = - 282.98 kJ mol¹¹) at a temperature of 400 °C: CO+0.502 → CO₂ In your calculations, consider the temperature-dependency of the molar heat capacities as follows: Cp (CO) = (21.75 +0.064 T-4.1.10-5T2)Jmol-¹K-1 Cp(O2) = (27.96 +0.004 T-1.7 10-7T²)Jmol¯¹K−¹ Cp (CO2)=(27.63 +0.005 T)Jmol-1K-1
1. A 50g sample of metal iron that was heated to 90 °C was dropped into a coffee cup calorimeter containing 200mL of water at room temperature of 25 °C. Applying the density of water (1g/mL) and specific heat capacity capacities of water and iron, determine the final temperature when the system reaches equilibrium.