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CHMA10H3 Lecture Notes - Lecture 9: Joule, Boiling Point, Kelvin

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violettiger441
24 Aug 2016
School
UTSC
Department
Chemistry
Course
CHMA10H3
Professor
Effiette Sauer

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CHMA10H3 Full Course Notes
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Document Summary

Sept 28 lec 8 chemical reactions and energy flows. Energy is obtained from hydrogen through an exothermic reaction with oxygen: The combustion of hydrogen does not produce carbon dioxide. H2 (g) + o2 (g) h2o(g) + 286 kj of energy. Most hydrogen is currently created by steam-methane reforming: Ch4 (g) + 2 h2o(g) co2 (g) + 4 h2 (g) The energy that keeps us alive (metabolism of foods) 5 c6h12o6 (s) + 6 o2 (g) 6 co2 (g) + 6 h2o(g) + energy. The unit used for measuring energy is the joule (j): one joule (1 j) is the energy required to lift an object exactly 1 m against the force of one. Newton (1 n): one newton is a force that will give a 1 kg object an acceleration of 1 m s 2 , so, 1 j = 1 kg m2 s 2 .

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Related Questions

  1. One suggestion for solving fuel-shortage problems is to use electric power (obtained from solar energy) to electrolyze water to form H2(g) and O2(g). The hydrogen could be used as a pollution-free fuel. In the following, enter ?H and ?G in kJ and ?S in J K-1 to two significant figures. Enter the quantities in the order that they appear. (a) Calculate ?H, ?S, and ?G in kJ for burning 1 kg of H2(g) to H2O(l) at 25 oC and 1 atm. (b) Calculate ?H, ?S, and ?G for burning 1 kg of n-octane(g) to H2O(l) and CO2(g) at 25oC and 1 atm.
Physical Chemistry

A)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.
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 0.392-g sample of bisphenol A (C15H16O2) in a bomb calorimeter containing 1140. g of water. The temperature increases from 25.00 °C to 27.40 °C. The heat capacity of water is 4.184 J g-1°C-1.
The molar heat of combustion is −7821 kJ per mole of bisphenol A.

C15H16O2(s) + 18 O2(g) ------>15 CO2(g) + 8 H2O(l) + Energy

Calculate the heat capacity of the calorimeter.
heat capacity of calorimeter =_________ J/°C

B)

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.

In an experiment, a 0.5574 g sample of benzil (C14H10O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.379×103 g of water. During the combustion the temperature increases from 26.36 to 28.99 °C. The heat capacity of water is 4.184 J g-1°C-1.
The heat capacity of the calorimeter was determined in a previous experiment to be 847.1 J/°C.
Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of benzil based on these data.
C14H10O2(s) + (31/2) O2(g) ------->5 H2O(l) + 14 CO2(g) + Energy
Molar Heat of Combustion = _________ kJ/mol



C)

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.

In an experiment, a 0.9900 g sample of β-D-fructose (C6H12O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.292×103 g of water. During the combustion the temperature increases from 21.82 to 24.12 °C. The heat capacity of water is 4.184 J g-1°C-1.
The heat capacity of the calorimeter was determined in a previous experiment to be 991.1 J/°C.
Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of β-D-fructose based on these data.
C6H12O6(s) + 6O2(g) -------> 6 H2O(l) + 6 CO2(g) + Energy
Molar Heat of Combustion = ____________ kJ/mol


All three problems are a set for one question on my homework, so please answer all three. Thank you so much!