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 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 90.16 grams of nickel to 98.98 °C and then drops it into a cup containing 84.90 grams of water at 22.80 °C. She measures the final temperature to be 30.48 °C. Water Metal sample Using the accepted value for the specific heat of nickel (See the References tool), calculate the calorimeter constant. e2003 ThomeonrkCoe 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. Thermometer 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 90.16 grams of nickel to 98.98 °C and then drops it into a cup containing 84.90 grams of water at 22.80 °C. She measures the final temperature to be 30.48 °C. Water Metal sample Using the accepted value for the specific heat of nickel (See the References tool), calculate the calorimeter constant. e2003 ThomeonrkCoe 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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ALab Data Temperature of cold water (°C) Temperature of hot water (°C) Volume of cold water (mL) Volume of hot water (mL) Final temperature after mixing (°C) Mass of cold water (g) Mass of hot water (g) Calorimeter constant (J/°C) 4.0 87.0 98.0 83.0 41.0 98.0 83.0 How to calculate the calorimeter constant Sm -
Reveiw steps of the calorimetry experiment. Describe how a calorimetry experiment is used to determine the enthalpy of a reaction. Gather the items to set up your calorimeter (coffee-cup, stir plate and stir bar, Vernier temperature probe, lid for coffee-cup) Pour 50.0 mL of DI water into the coffee-cup calorimeter. You will be preparing 50.0 mL of a 1.0 M solution of sodium nitrate solution. Using the Vernier temperature probe, record the initial temperature of your DI water. Weigh out the mass of sodium nitrate needed for your solution and pour it into the calorimeter. Immediately begin collecting temperature data. Repeat multiple times.
Fill in the blank: Dilution ______________ the percent dissociation of the solution.
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. Water Thermometer Metal sample 2003 Thomson-Brooks/Cole 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 100.00 grams of nickel to 98.10 °C and then drops it into a cup containing 79.36 grams of water at 23.62 °C. She measures the final temperature to be 32.36 °C. Using the accepted value for the specific heat of nickel (See the References tool), calculate the calorimeter constant. Calorimeter Constant = J/°C
5575082893418928809969212&elSBN=9781305657571&... Tp Q Search this co References Use the References to access important values if needed for this question. A student determines the heat of dissolution of solid cobalt(II) chloride using a coffee-cup calorimeter of negligible heat capacity. When 1.58 g of CoCl,(s) is dissolved in 101.00 g of water, the temperature of the solution increases from 25.00 to 27.42 °C. Based on the student's observation, calculate the enthalpy of dissolution of CoCl,(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. AH dissolution kJ/mol Submit Answer
Calculate the enthalpy of solution (AH for the dissolution) per mole of CaCl, (refer to Exercise 5.25). Exercise 5.25: Dissolving 3.0 g of CaCl2(s) in 150.0 g of water in a calorimeter (Figure 5.12) at 22.4 °C causes the temperature to rise to 25.8 °C. What is the approximate amount of heat involved in the dissolution, assuming the specific heat of the resulting solution is 4.18 J/g °C? Is the reaction exothermic or endothermic? heat: [ Select] exothermic vs endothermic: [Select] enthalpy: [ Select ] a 99+
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. Themeter Mod 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 92.55 grams of zinc to 97.73 °C and then drops it into a cup containing 78.30 grams of water at 21.37 °C. She measures the final temperature to be 28.88 °C. Using the accepted value for the specific heat of zinc (See the References tool), calculate the calorimeter constant. Calorimeter Constant = 3/°C Submit Answer Retry Entire Group 8 more group attempts remaining
Ignition wires heat Thermometer Stirrer A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. sample 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. %3D Water In the laboratory a student burns a 0.596-g sample of acetylsalicylic acid (C,H3O4) in a bomb calorimeter containing 1090. g of water. The temperature increases from 24.40 °C to 26.80 °C. The heat capacity of water is 4.184 J gl°C 1 The molar heat of combustion is -3869 kJ per mole of acetylsalicylic acid. C,H3O4(s) + 9 O2(g) - →9 CO2(g) + 4 H20(1) + Energy Calculate the heat capacity of the calorimeter. Burning sample Insulated Sample dish Steel outside chamber bomb heat capacity of calorimeter = J/°C Combustion (bomb) calorimeter.
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
A 21.42g sample of an unknown metal was heated to 99.5ºC, and the added to 50.00g of water contained in a foam coffee cup. The initial temperature of the water was 20.5ºC, and the final temperature of the metal and water was 25.1ºC. The calorimeter constant for the coffee-cup calorimeter was 13.5 J/ºC. What was the specific heat of the metal? * the answer is 0.64 J/gºC, but I need to know how to get there
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
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 to 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.