7. For the following scenarios what is the metal?a. A piece of metal weighing 59.047 g was heated to 100.0 °C and then putit into 100.0 mL of water (initially at 23.7 °C). The metal and water wereallowed to come to an equilibrium temperature, determined to be 27.8°C. Assuming no heat lost to the environment, calculate the specific heatof the metal.platinumniobiumvandiumtitaniumC (kJ/kg K)0.130.270.390.54b. A 25.6 g piece of metal was taken from a beaker of boiling water at 100.0 °C and placed directlyinto a calorimeter holding 100.0 mL of water at 25.0 °C. The calorimeter heat capacity is 1.23 J/K.Given that the final temperature at thermal equilibrium is 26.2 °C, determine the specific heatcapacity of the metal.

Given,a, mass of metal = 59.047 gInitial temperature of metal = 100.0 oCvolume of water = 100.0…

Answered: 7. For the following scenarios what is…

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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4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
In a simple calorimeter, a piece of metal weighing 48.67 g was heated to 120.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal. Is this process endothermic or exothermic? Explain. Show Your Work
A certain chemical reaction releases 269. kJ of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 3.21 J of heat energy to raise the temperature of this calorimeter by 1 °C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 5.0 °C. How would you calculate the number of moles of reactant that were consumed? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols. moles consumed = x10 010 X Ś
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A student followed the procedure in this experiment, using 50.00 mL of 2.00 molar HCl and 51.00 mL of 2.00 molar NaOH both solutions having an initial temperature of 22.7 oC. After mixing, a maximum temperature of 32.2 oC is measured. The final mass of the mixture was found to be 104.84 grams. For this problem, assume the specific heat of the solution is 4.18 J/g oC. Report all answers with the proper number of significant figures. What is the heat transferred by this reaction, in Joules?
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Ice at 0.0 °C is placed in a Styrofoam cup containing 372. g of a soft drink at 15.4 °C. The specific heat of the drink is about the same as that of water. Some ice remains after the ice and soft drink reach an equilibrium temperature of 0.0 °C. Determine the mass of ice that has melted. Ignore the heat capacity of the cup. (Hint: It takes 334 J to melt 1 g of ice at 0.0 °C.) Be sure your answer has the correct number of significant digits. Note: Reference the Phase change properties of pure substances table for additional information. 1 6.D g x10 Ś
4. Aluminum metal melts at 658.5°C. What would be the final temperature if 28.0 grams of solid aluminum at this temperature were placed into 520 grams of liquid aluminum at 1000.0°C? The heat of fusion for aluminum is 396 J/ -1 -1 g, and the specific heat of liquid aluminum is 0.481 J-g`¹deg-¹. (Note: this is the aluminum analog to the process you just did in lab!)
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19. A peice of titanium metal with a mass of 20.8 g is heated in boiling water to 99.5°C and the dropped into a coffee cup calorimeter containing 75.0 g water at 21.7°C. When the thermal equilibrium is reached, the final temperature is 24.3°C. Calculate the specific heat capacity of titanium. 15. The enthalphy of fusion (melting) of water is 6.0 kJ/mol. CAlculate the quantity of energy that must be transffered to melt 25.0 g H2O at 0°C. ps. pls answer the number 19 if you will just answer one question. But if you can answer two questions pls answer it. Im begging youu :<

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