A calorimeter contains 140 g water. The calorimeter and the water inside are both at 24 °C. A piece of metal weighing 45 g was heated to 98 °C and then put into the water inside the calorimeter. The equilibrium temperature was determined to be 35 °C. Assuming no heat is lost o the environment, calculate the specific heat of the metal. Calorimeter constant: 130 J°C-1 Specific heat of water: 4.184 J°C-1g*1 O A. 2.78 J°C*!g*1 O B. 2.26 J°C*!g*1 O. 2.37 J°C*!g°1 O D. 1.93 J°C"lg*1 Q E. 1.81 J°C*1g*1

A calorimeter contains 140 g water. The calorimeter and the water inside are both at 24 °C. A piece of metal weighing 45 g was heated to 98 °C and then put into the water inside the calorimeter. The equilibrium temperature was determined to be 35 °C. Assuming no heat is lost o the environment, calculate the specific heat of the metal. Calorimeter constant: 130 J°C-1 Specific heat of water: 4.184 J°C-1g1 O A. 2.78 J°C!g1 O B. 2.26 J°C!g1 O. 2.37 J°C!g°1 O D. 1.93 J°C"lg1 Q E. 1.81 J°C1g*1

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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A calorimeter contains 140 g water. The calorimeter and the water inside are both at 24 °C. A piece of metal weighing 45 g was heated to 98 °C and then put into the water inside the calorimeter. The equilibrium temperature was determined to be 35 °C. Assuming no heat is lost to the environment, calculate the specific heat of the metal. Calorimeter constant: 130 J°C-1 Specific heat of water: 4.184 J°C*g1 O A. 2.26 J°C-lg1 O B. 2.78 J°Clg-1 oc.1.81 J°Cg1 O D.193 J°C-lg1 O E. 2.37 J°C-1g-1
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40.0 g of an unknown metal at 100.0°C is added to 50.0 g of water at 30.0°C. When the system reaches equilibrium, the temperature is 34.5°C. What is the specific heat of the metal?
12. In an experiment, 5.260 g of potassium hydroxide is mixed with a dilute solution of hydrochloric acid. A neutralization reaction occurs. The hydrochloric acid is in excess. The specific heat capacity for water is 4.184 J/g. °C. The following data are obtained: Initial temperature of HCl Volume of HCl Final temperature of solution after mixing Calculate the molar enthalpy of reaction (AH₂) for potassium hydroxide. 24.5 °C 200.0 mL 31.4 °C
Simple Calorimetry. A piece of solid aluminum at 15.0°C is immersed in 12.3 g of nitrogen gas which is initially at 51.1°C and the system is allowed to equilibrate. Given that the specific heat of solid aluminum is 0.908 J/K/g and the specific heat of nitrogen gas is 1.0 J/K/g, what is the mass of the piece of solid aluminum if the final temperature is 34.7°C?
A 50.0 mL sample of a 1.00 MM solution of CuSO4CuSO4 is mixed with 50.0 mL of 2.00 MM KOHKOH in a calorimeter. The temperature of both solutions was 24.6 oCoC before mixing and 32.8 oCoC after mixing. The heat capacity of the calorimeter is 12.1 J/K. From these data, calculate ΔHΔH for the process: CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M)CuSO4(1M)+2KOH(2M)→Cu(OH)2(s)+K2SO4(0.5M) Assume that the specific heat and density of the solution after mixing are the same as those of pure water and that the volumes are additive.
2. A calorimeter contains 100.0 g of water at 39.8 °C. A 12.78 g object at 100.0 ºC is placed inside the calorimeter. When equilibrium has been reached, the new temperature of the water and metal object is 40.6 °C. What is the specific heat of the metal?
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
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?
The heat capacity of an object indicates how much energy that object can absorb for a given increase in that object's temperature. In a system in which two objects of different temperatures come into contact with one another, the warmer object will cool and the cooler object will warm up until the system is at a single equilibrium temperature. Note the difference between the terms molar heat capacity, which has units of J/(mol-K). and specific heat, which has units of J/(g-K). Remember to use 3 significant figures for all answers unless stated otherwise in the problem. Common issues with this problem involve entering units incorrectly into the answer field. Please check this help website for a refresher on how to enter units in Mastering Chemistry: http://help.pearsoncmg.com/mastering/student/standalone/TopicsStudent/acceptable units list.htm The margin of error is 2%. Part A A volume of 75.0 mL of H₂O is initially at room temperature (22.0 °C). A chilled steel rod at 2.00 °C is placed…
Calculate the energy content (in calories) of a 1.00 g of product that is placed inside a calorimeter having a heat capacity of 950 J/K. Data from the calorimeter indicated that the 3.0 L surrounding water had initial and final temperatures of 18.0 °C and 47.5 °C, respectively. Specific heat capacity of water: 4.18 J/g-K a. 2.6x10^4 cal b. 9.5x10^4 cal c. 8.8x10^4 cal d. 7.3x10^4 cal