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)
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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-10C. (Relative atomic mass
of C=12; 0=16; H=1)
5. The molar mass of enthalpy of combustion of glucose, C6H1206 is -2803 kJ. A mass
of 1.00 g glucose is combusted in a bomb calorimeter. If the calorimeter contains
875 g H20 and the bomb has a heat capacity of 475 J°C, what is the temperature
increase of the bomb calorimeter? The specific heat capacity of water is 4.184 J K-1
g1 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 an
experiment 4.34 g of this compound was burnt completely and the heat evolved
raised the temperature of y g of water from 27.5 °C to 45.5 °C.[Specific heat
capacity 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 of
250 cm3 water contained in a copper beaker by 20.0 °C. [Specific heat capacity of
solution = 4.18 Jg-1 °C1; density of solution = 1.0 g cm-3]
2
TUTORIAL 2 CHM271 PRINCIPLES OF PHYSICAL CHEMISTRY
i)
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 cm3
water in the same copper beaker.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6cfc2e1a-b55c-4430-b159-5e3bb63a6548%2Feee6e386-6a07-4ac7-8cb3-3c642517f522%2Fgqpwyne_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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-10C. (Relative atomic mass
of C=12; 0=16; H=1)
5. The molar mass of enthalpy of combustion of glucose, C6H1206 is -2803 kJ. A mass
of 1.00 g glucose is combusted in a bomb calorimeter. If the calorimeter contains
875 g H20 and the bomb has a heat capacity of 475 J°C, what is the temperature
increase of the bomb calorimeter? The specific heat capacity of water is 4.184 J K-1
g1 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 an
experiment 4.34 g of this compound was burnt completely and the heat evolved
raised the temperature of y g of water from 27.5 °C to 45.5 °C.[Specific heat
capacity 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 of
250 cm3 water contained in a copper beaker by 20.0 °C. [Specific heat capacity of
solution = 4.18 Jg-1 °C1; density of solution = 1.0 g cm-3]
2
TUTORIAL 2 CHM271 PRINCIPLES OF PHYSICAL CHEMISTRY
i)
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 cm3
water in the same copper beaker.
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