6. A 40.00 g sample of water at 22.00°C is put in a calorimeter. After 60.00g of water at 65.00°C is added to the calorimeter, the mixture is stirred,and the final temperature is 47.00°C. Calculate the heat capacity of thecalorimeter in calfC.7. A piece of metal weighing 7.00 g is heated to 93.0°C and placed into thecalorimeter described in the previous problem. The calorimeter contains 25.0g of water at 30.0°C. If the final temperature of the water is 33.0°C, cal-culate the specific heat of the metal in cal/g °C.

(6) Given - Mass of water at 22.00°C = 40.00 g Mass of water at 65.00°C = 60.00 g Final…

6. A 40.00 g sample of water at 22.00°C is put in a calorimeter. After 60.00 g of water at 65.00°C is added to the calorimeter, the mixture is stirred, and the final temperature is 47.00°C. Calculate the heat capacity of th. calorimeter in calPC. 7. A piece of metal weighing 7.00 g is heated to 93.0°C and placed into the calorimeter described in the previous problem. The calorimeter contains 25. g of water at 30.0°C. If the final temperature of the water is 33.0°C, cal- ifin hoot off the metal in cal/g °C. 0uloto

6. A 40.00 g sample of water at 22.00°C is put in a calorimeter. After 60.00 g of water at 65.00°C is added to the calorimeter, the mixture is stirred, and the final temperature is 47.00°C. Calculate the heat capacity of th. calorimeter in calPC. 7. A piece of metal weighing 7.00 g is heated to 93.0°C and placed into the calorimeter described in the previous problem. The calorimeter contains 25. g of water at 30.0°C. If the final temperature of the water is 33.0°C, cal- ifin hoot off the metal in cal/g °C. 0uloto

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

A 22.1g piece of aluminum (which has a molar capacity of 24.03 J/oC.mol) is heated to 82.4oC and dropped into a calorimeter containing water (specific heat capacity of water is 4.18J/goC) initially at 22.3oC. The final temperature of the water is 25.8oC. Ignoring significant figures, calculate the mass of the water in the calorimeter.
4 Having just invented a new type of calorimeter, Dr. Campbell needs to determine the heat capacity of the calorimeter. She carries out the following experiment to do this: She puts 20.0 grams of water in her empty calorimeter and it is allowed to stabilize at a temperature of 25.0ºC. She then adds 32.035 grams of water at a temperature of 83.2ºC to the calorimeter. After a few minutes the final temperature of the calorimeter stabilizes at 41.6ºC. Based on this experiment, what is the heat capacity of her calorimeter assuming units of J/ºC? Enter your answer with at least 3 sig figs.
A 1.75 g sample of zinc metal is reacted with 128 g of 1.10 M hydrochloric acid solution in a constant-pressure calorimeter. The resulting solution changes in temperature from 22.58 °C to 22.97 °C. The hydrochloric acid is in excess. Based on this information, and estimating the solution's heat capacity as 4.18 Jg1 °C, what is the amount of heat, in joules, transferred in this reaction?
When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
A 79.1 g sample of an unknown solid is heated to 62.6ºC and placed into a calorimeter containing 92.1 g of water at 22ºC. If the final temperature of the solid sample and the water is 32.5ºC, what is the specific heat of the solid? Please provide your final answer rounded to two decimal places.
10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C
A 5.1-gram piece of gold jewelry isremoved from water at 100.0°C and placed in a coffee-cup calorimeter containing 16.9 gof water at 22.5°C (specific heat of water is 4.184 J/g · °C). The equilibrium (final)temperature of the water and jewelry is 23.2°C. The calorimeter constant is known fromcalibration experiments to be 1.54 J/°C. What is the specific heat (in J/g · °C) of this pieceof jewelry? If the tabulated value of the specific heat of gold is 0.129oC, is the jewelrypure gold?
A 56.1 g sample of polystyrene, which has a specific heat capacity of 1.880 J-g °C-1 is put into a calorimeter (see sketch at right) that contains 250.0 g of water. The temperature of the water starts off at 24.0 °C. When the temperature of the water stops changing it's 29.8 °C. The pressure remains constant at 1 atm. Calculate the initial temperature of the polystyrene sample. Be sure your answer is rounded to the correct number of significant digits. °C thermometer. insulated container water sample. a calorimeter 區 OU Ar
Please don't provide handwritten solution ...
A chemist carefully measures the amount of heat needed to raise the temperature of a 0.34 kg sample of C,H¸0 from -1.5 °C to 18.1 °C. The experiment shows that 1.09 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H,O? Round your answer to 2 significant digits. J• mol -1 1 ·K x10
A 44.0 g sample of unknown metal at 99.0°C was placed in a constant-pressure calorimeter containing 80.0 g of water at 24.0°C, the final temperature of the system was found to be 28.4°C. Calculate the specific heat of the metal.
A student reacts 2.0 moles A and 4.0 moles of B in an insulated container. The reaction takes place in water (50.0 g), in a coffee cup. The water gains heat, raising its temperature 23.6°C (AT). Water has a specific heat capacity of 4.184 J/g C. A + 2B 3 C AHRXN = ? 1 a. Energy is absorbed by the water. What is qWATER? b. Energy is released by the reaction. What is qRXN? (this one is easy) c. How much heat per mol of A (or per 2 mol of B), by the reaction (AHRXN)? d. In another reaction, a student reacts 15.2 moles of B with excess A. What is the heat that comes out of his second reaction (qRXN-2)? use dimensional analysis +