4. 1.922 g methanol (CH3OH) was burned in a constant-volume bomb calorimeter.Consequently, the temperature of the water rose by 4.20 °C. If the quantity ofwater surrounding the calorimeter was exactly 2000 g and the heat capacity of thecalorimeter was 2.02 kJ°C1, calculate the molar heat of combustion of methanol.Assume the specific heat capacity of CH3OH is 4.184 Jg-10C. (Relative atomic massof C=12; 0=16; H=1)5. The molar mass of enthalpy of combustion of glucose, C6H1206 is -2803 kJ. A massof 1.00 g glucose is combusted in a bomb calorimeter. If the calorimeter contains875 g H20 and the bomb has a heat capacity of 475 J°C, what is the temperatureincrease of the bomb calorimeter? The specific heat capacity of water is 4.184 J K-1g1 and the molar mass of glucose is 180.2 g mol1.6. The heat of combustion of liquid ethylene glycol, C2H6O2 is -1189.2 kJ/mol. In anexperiment 4.34 g of this compound was burnt completely and the heat evolvedraised the temperature of y g of water from 27.5 °C to 45.5 °C.[Specific heatcapacity of water = 4.2 J g1°C 1]i) Write the thermochemical equation for the heat of combustion of C2H6O20)ii) Calculate the value of y (mass of water used)7. The heat evolved from the combustion of 0.94g ethanol raises the temperature of250 cm3 water contained in a copper beaker by 20.0 °C. [Specific heat capacity ofsolution = 4.18 Jg-1 °C1; density of solution = 1.0 g cm-3]2TUTORIAL 2 CHM271 PRINCIPLES OF PHYSICAL CHEMISTRYi)What is the enthalpy of combustion per mol of ethanol?ii)Calculate the temperature rise when 1.50 g ethanol is used to heat 500 cm3water in the same copper beaker.

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4. 1.922 g methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature of the water rose by 4.20 °C. If the quantity of water surrounding the calorimeter was exactly 2000 g and the heat capacity of the calorimeter was 2.02 KJ°C1, calculate the molar heat of combustion of methanol. Assume the specific heat capacity of CH3OH is 4.184 Jg 1°C1. (Relative atomic mass of C=12; 0=16; H=1)

4. 1.922 g methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature of the water rose by 4.20 °C. If the quantity of water surrounding the calorimeter was exactly 2000 g and the heat capacity of the calorimeter was 2.02 KJ°C1, calculate the molar heat of combustion of methanol. Assume the specific heat capacity of CH3OH is 4.184 Jg 1°C1. (Relative atomic mass of C=12; 0=16; H=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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