4. Bomb calorimetry was performed to determine the calorific value for a sample of edible oil. The following data were obtained and recorded: mass of the oil sample heat capacity of the calorimeter volume of water in the calorimeter initial temperature final temperature = 1.75 g = 1.3 kJ/ºC = 950 ml = 25.8 °C = 30.3 °C Compute for the calorific value of the sample in Cal/g.

4. Bomb calorimetry was performed to determine the calorific value for a sample of edible oil. The following data were obtained and recorded: mass of the oil sample heat capacity of the calorimeter volume of water in the calorimeter initial temperature final temperature = 1.75 g = 1.3 kJ/ºC = 950 ml = 25.8 °C = 30.3 °C Compute for the calorific value of the sample in Cal/g.

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

100.0 mL of cold water at 20.5 oC was poured into a styrofoam coffee cup calorimeter. After adding 100.0 mL of hot water at 30.5 oC and mixing it thoroughly, the temperature of the mixture was found to 24.7 oC. Find the heat capacity of the calorimeter. [Specific heat capacity of water is 4.184 J/goC. Assume density of water is 1.0 g/mL at both temperatures.]
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 -
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
thermometer. insulated container A sample of quartz, which has a specific heat capacity of 0.730 J-goC, is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The quartz sample starts off at 90.0 °C and the temperature of the water starts off at 25.0 °C. When the temperature of the water stops changing it's 27.1 °C. The pressure remains constant at 1 atm. water Calculate the mass of the quartz sample. Be sure your answer is rounded to 2 significant digits. 0 x10 X ? a sample a calorimeter do F
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 45.90 g sample of pure copper is heated in a test tube to 99.40°C. The copper sample is then transferred to a calorimeter containing 61.04 g of deionized water. The water temperature in the calorimeter rises from 24.39°C to 29.10°C. The specific heat capacity of copper metal and water are J and 4.184 J 0.387 respectively. g. °C g. °C Assuming that heat was transferred from the copper to the water and the calorimeter, determine the heat capacity of the calorimeter. Heat capacity of calorimeter-
An 27.301g piece of metal is heated in a hot water bath at 98.5°C and then transferred to a coffee-cup calorimeter containing 50.0mL of water. The initial water temperature was 24.0°C and the final water temperature was 26.2°C. Determine the specific heat of the metal (Cmetal). Ccal = 21.0J/°C & Cwater = 4.184 J/g*°C. Report your answer to 3 sf and in J/g*°C. %3D
thermometer A 53.6 g sample of brass, which has a specific heat capacity of 0.375 J'g.°C', is put into a calorimeter (see sketch at right) that contains 300.0 g of water. The temperature of the water starts off at 19.0 °C. When the temperature of the water stops changing it's 20.2 °C. The pressure remains constant at 1 atm. insulated container water Calculate the initial temperature of the brass sample. Be sure your answer is rounded to 2 significant digits. sample - a calorimeter Continue Submit Assignment 02021 McGraw Hill LLC A Rights Reserved. Terms of Use Privacy Center I Accessibility
DUE NOW. Please answer it neatly, correctly, and with DETAILED solutions. Thanks!