In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 90.62 grams of zinc t 97.68 °C and then drops it into a cup containing 84.45 grams of water at 23.94 °C. She measures the final temperature to be 30.58 °C. Using the accepted value for the specific heat of zinc (See the References tool), calculate the calorimeter constant. Calorimeter Constant = | J/°C.

In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 90.62 grams of zinc t 97.68 °C and then drops it into a cup containing 84.45 grams of water at 23.94 °C. She measures the final temperature to be 30.58 °C. Using the accepted value for the specific heat of zinc (See the References tool), calculate the calorimeter constant. Calorimeter Constant = | J/°C.

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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General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning A 2.50 g sample of powdered zinc is added to 100.0 mL of a 2.00 M aqueous solution of hydrobromic acid in a calorimeter. The total heat capacity of the calorimeter and solution is 448 J/K. The observed increase in temperature is 21.1 K at a constant pressure of one bar. Calculate the standard enthalpy of reaction using these data. Zn(s) + 2 HBr(aq) ZnBr, (aq) + H,(g) AHan = kJ/mol rxn Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry| Publisher: University Science Books étv MacBook Air DU 888 F7 FO F4 % T0 delet %23 8.
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.
In this experiment you will place a sample of your salt in water in a constant pressure calorimeter. You will determine the enthalpy change for the dissociation of your salt, Delta Hdiss. A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃ and the final temperature was 27.086365℃. What is the number of moles of SrCl2? 4.368 g SrCl2 x ( 1 mol SrCl2 / 123.073 g SrCl2 ) = 0.035491131 mol SrCl2 a. 0.035491 mol SrCl2 b. none of these c. 0.035 mol SrCl2 d. 0.03 mol SrCl2 e. 0.0355 mol SrCl2 f. 0.04 mol SrCl2 g. 0.035491131 mol SrCl2 h. 0.03549 mol SrCl2
thermometer A 57.4 g sample of glass is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The glass sample starts off at insulated 86.3 °C and the temperature of the water starts off at 18.0 °C. When the temperature of the water stops changing it's 24.1 °C. The container pressure remains constant at 1 atm. water Calculate the specific heat capacity of glass according to this experiment. Be sure your answer is rounded to the correct number of significant digits. sample a calorimeter
make sure that the answer is in the correct number of significant digits
Let's use our knowledge of constant volume (bomb) calorimetry to determine the heat energy in a given food sample, say a hamburger. A typical hamburger has a serving size of 105 g and consists of approximately 20% protein (21.0 g), 33% fat (34.7 g), and 47% carbohydrate (49.3 g). Assume that the heat capacity of the bomb calorimeter is 8.39 kJ K-¹, and the increase in water temperature was 13.2 K. Q5.38 Homework Unanswered How many Calories (Cal) are in the hamburger described above? Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. 2.5E5 for 2.5 x 105) Type your numeric answer and submit Unanswered • 4 attempts left Submit
Chemistry 14) A 60.0 mL quantity of 0.80 M HCI is mixed with 60.0 mL of 0.80 M KOH in a constant pressure calorimeter with negligible heat capacity. If the initial temperatures of both solutions are equal to 20.24°C. Calculate the heat change of the neutralization reaction if the final temperature of the mixture is 30.0°C. Assume that the densities and specific heats of the solutions are the same as those of water (1.00 g/mL and 4.184 J/g °C, respectively). Note: this point is worth 10 points. A) + 4900.3 J B)-1171.2 J C)-2450.15 J D)-4900.3 J
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.508-g sample of benzil (C14H1002) in a bomb calorimeter containing 1060. g water. The temperature increases from 24.70 °C to 27.80 °C. The specific heat capacity of water is 4.184 J gl°C1. The combustion enthalpy is -6784 k]/mol benzil. C14H1002(s) + 31/2 02(g) →14 CO2(g) + 5 H20(I) A,H° = -6784 kJ/mol %3D Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/C
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. Thermometer Metal sample ©2003 Thomson-Brooks/Co Stirring rod Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant. One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 93.37 grams of zinc to 98.36 °C and then drops it into a cup containing 81.25 grams of water at 21.46 °C. She measures the final temperature to be 28.84 °C. Using the accepted value for the specific heat of zinc (See the References tool), calculate the calorimeter constant. Calorimeter Constant = J/°C
You accidentally forgot to measure the mass of the octane that you transferred in the crucible. You already started the calorimeter and it is too late to stop the equipment. Is it still possible to calculate the energy (in Joules) of octane?