In an experiment, a 1.3440 g sample of dimethyl oxalate (C4H6 O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.383 x 103 g of water. During the combustion the temperature increases from 25.58 to 28.50 °C. The heat capacity of water is 4.184 J. g. C¹. The heat capacity of the calorimeter was determined in a previous experiment to be 989.5 J. "C¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of dimethyl oxalate based on these data. C4H6O4(s)+(7/2)O2(g) → 3H2O(l) + 4CO2(g) +Energy Molar Heat of Combustion = kJ/mol

In an experiment, a 1.3440 g sample of dimethyl oxalate (C4H6 O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.383 x 103 g of water. During the combustion the temperature increases from 25.58 to 28.50 °C. The heat capacity of water is 4.184 J. g. C¹. The heat capacity of the calorimeter was determined in a previous experiment to be 989.5 J. "C¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of dimethyl oxalate based on these data. C4H6O4(s)+(7/2)O2(g) → 3H2O(l) + 4CO2(g) +Energy Molar Heat of Combustion = kJ/mol

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 100AE

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Nitrogen gas (2.75 L) is confined in a cylinder under constant atmospheric pressure (1.01 105 pascals). The volume of gas decreases to 2.10 L when 485 J of energy is transferred as heat to the surroundings. What is the change in internal energy of the gas?
The enthalpy of combustion of diamond is -395.4 kJ/mol. C s, dia O2 g CO2 g Determine the fH of C s, dia.
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A sample of sucrose, C12H22O11, is contaminated by sodium chloride. When the contaminated sample is burned in a bomb calorimeter, sodium chloride does not burn. What is the percentage of sucrose in the sample if a temperature increase of 1.67C is observed when 3.000 g of the sample are burned in the calorimeter? Sucrose gives off 5.64103kJ/mol when burned. The heat capacity of the calorimeter and water is 22.51 kJ/C.
An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g)+3O2(g)2H2O(l)+2SO2(g);H=1124kJ The density of sulfur dioxide at 25C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/(mol C). (a) How much heat would be evolved in producing 1.00 L of SO2 at 25C and 1.00 atm? (b) Suppose heat from this reaction is used to heat 1.00 L of the SO2 from 25C to 500C for its use in the next step of the process. What percentage of the heat evolved is required for this?
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When solid iron burns in oxygen gas (at constant pressure) to produce Fe2O3(s), 1651 kJ of heat is released for every 4 mol of iron burned. How much heat is released when 10.3 g Fe2O3(s) is produced (at constant pressure)? What additional information would you need to calculate the heat released to produce this much Fe2O3(s) if you burned iron in ozone gas, O3(g), instead of O2(g)?
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A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25.00C to 33.73C. If the heat capacity of the calorimeter and contents was 9.63 kJ/C, what is the value of q for burning 1.00 mol of ethanol at constant volume and 25.00C? The reaction is C2H5OH(l)+3O2(g)2CO2(g)+3H2O(l) Is q equal to U or H?
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