A bomb calorimetry experiment is performed with xylose, CSH10O5 (S), as the combustible substance. The data obtained are: mass of xylose burned: 1.764g; heat capacity of calorimeter: 4.728 kJ/"C; initial calorimeter temperature: 23.29°C; final calorimeter temperature 27.19°C. What is the heat of combustion of xylose, in kilojoules per mole? Lütfen birini seçin: O a. -1.57x10" kJ/mol O b.-5.64x10* kJ/mol O c -3.17x10" kJ/mol O d. -3.34x10ª kJ/mol O e. -2.38x10 kJ/mol

A bomb calorimetry experiment is performed with xylose, CSH10O5 (S), as the combustible substance. The data obtained are: mass of xylose burned: 1.764g; heat capacity of calorimeter: 4.728 kJ/"C; initial calorimeter temperature: 23.29°C; final calorimeter temperature 27.19°C. What is the heat of combustion of xylose, in kilojoules per mole? Lütfen birini seçin: O a. -1.57x10" kJ/mol O b.-5.64x10* kJ/mol O c -3.17x10" kJ/mol O d. -3.34x10ª kJ/mol O e. -2.38x10 kJ/mol

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

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). First, a 7.000 g tablet of benzoic acid (CH₂CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 15.00 °C to 53.26 °C over a time of 12.3 minutes. Next, 5.420 g of acetylene (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 74.42 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy ΔΗ. per mole of…
A 0.4554g sample of sucrose (C12H22O11) is burned in a calorimeter which has a calorimeter constant of 333 J/℃. The calorimeter contains 500.0g of water. If the temperature of the water and calorimeter increase by 3.093℃, a) Calculate the heat given off by the burning sucrose. b) Calculate the molar heat of combustion of sucrose (that is, the heat which would be given off by the combustion of one mole of sucrose).
Fructose, C6H12O6(s), is a sugar closely related to glucose. A 0.755 g sample of fructose was combusted with excess oxygen in a bomb calorimeter, containing 500.0 g of water. The heat capacity of the empty calorimeter was 208 J/K. The temperature of the calorimeter and the water rose from 22.00°C to 27.12°C due to the combustion reaction, which formed CO₂(g) and liquid water. What is the energy change, AU (in kJ), for the combustion of one mole of fructose under these conditions? O +254 O-15600 -2810 +520 -804
When 9.1 g of a hydrocarbon is combusted in a bomb calorimeter the temperature of the calorimeter increases from 23.8 C to 53.5 C. The calorimeter contains 731 g of water and the heat capacity of the bomb is 872 J/ C. Please calculate q rxn, in kJ, for the combustion of the hydrocarbon.
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1400. g of water (see sketch at right). First, a 5.000 g tablet of benzoic acid (CH-CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 21.00 °C to 42.00 °C over a time of 8.5 minutes. Next, 5.190 g of ethylene (C₂H4) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 21.00 °C to 63.35 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. exothermic C₂H₂(g) + 30₂(g) → 2CO₂(g) + 2H₂O(g) Be…
At constant volume, the heat of combustion of a particular compound is -3916.0 kJ/mol. When 1.329 g of this compound (molar mass = 166.62 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter, including its contents, rose by 7.549 "C. What is the heat capacity (calorimeter constant) of the calorimeter? calorimeter constant: kJ/ "C
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1500. g of water (see sketch at right). First, a 5.000 g tablet of benzoic acid (C6H-CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 14.00 °C to 33.17 °C over a time of 6.8 minutes. Next, 4.040 g of acetylene (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 14.00 °C to 39.42 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy ΔΗ, per mole of…
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). First, a 5.000 g tablet of benzoic acid (CH-CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 22.00 °C to 42.76 °C over a time of 9.6 minutes. Next, 5.990 g of ethane (C₂H) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 22.00 °C to 71.14 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy ΔΗ per mole of C₂H6.…
Fructose, C6H12O6(s), is a sugar closely related to glucose.. A 0.755 g sample of fructose was combusted with excess oxygen in a bomb calorimeter, containing 500.0 g of water. The heat capacity of the empty calorimeter was 208 J/K. The temperature of the calorimeter and the water rose from 22.00°C to 27.12°C due to the combustion reaction, which formed CO2(g) and liquid water. What is the energy change, AU (in kJ), for the combustion of one mole of fructose under these conditions? -15600 -2810 +520 +254 -804
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1500. g of water (see sketch at right). First, a 6.500 g tablet of benzoic acid (CH₂CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 18.00 °C to 44.66 °C over a time of 14.6 minutes. Next, 4.910 g of ethanol (C₂H5OH) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 18.00 °C to 40.44 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy AHxn per mole of…
In an experiment, a 0.5002 g sample of tridecanedioic acid ( C13 H24 O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.165 × 10³ g of water. During the combustion the temperature increases from 21.99 to 24.52 °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 904.0 J. °C¯¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of tridecanedioic acid based on these data. C13H24 O4(s) + 17O2 (g) → 12H₂O(l) + 13CO2 (g) + Energy kJ/mol Molar Heat of Combustion =
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). First, a 7.500 g tablet of benzoic acid (CH₂CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 18.00 °C to 51.74 °C over a time of 14.9 minutes. Next, 4.510 g of ethane (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 18.00 °C to 53.35 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy ΔΗ per mole of C₂H6.…