Ignition wires Thermometer Stirrer heat A sample of solid anthracene (C14H10) that weighs 0.4927 g is burned in an excess of oxygen to CO,(g) and H,0(,) in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.120 °C. The heat capacity of the calorimeter and its contents is known to be 9.207×10³ J K!. sample (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank. Water Based on this experiment: (b) Assuming that AH° is approximately equal to AE, calculate the standard enthalpy change for the combustion of 1.000 mol of anthracene to CO2(g) and H,0(,). kJ mol¯1 Insulated outside chamber Sample dish Burning sample Steel bomb Combustion (bomb) calorimeter. (c) Calculate the standard enthalpy of formation per mole of anthracene, using the following for the standard enthalpies of formation of CO2(g) and H20(,). AHº H2O (,) = -285.83 kJ mol"!; AHº CO,(g) = -393.51 kJ mol"! kJ mol¯!

Ignition wires Thermometer Stirrer heat A sample of solid anthracene (C14H10) that weighs 0.4927 g is burned in an excess of oxygen to CO,(g) and H,0(,) in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.120 °C. The heat capacity of the calorimeter and its contents is known to be 9.207×10³ J K!. sample (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank. Water Based on this experiment: (b) Assuming that AH° is approximately equal to AE, calculate the standard enthalpy change for the combustion of 1.000 mol of anthracene to CO2(g) and H,0(,). kJ mol¯1 Insulated outside chamber Sample dish Burning sample Steel bomb Combustion (bomb) calorimeter. (c) Calculate the standard enthalpy of formation per mole of anthracene, using the following for the standard enthalpies of formation of CO2(g) and H20(,). AHº H2O (,) = -285.83 kJ mol"!; AHº CO,(g) = -393.51 kJ mol"! 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

The earth's atmosphere is 78% nitrogen by volume. Write and solve a proportion to find the amount of nitrogen in a tank containing 425 cubic meters of air.
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300.g of water (see sketch at right). First, a 6.000g tablet of benzoic acid C6H5CO2H is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of /26.454kJg .) The temperature of the water is observed to rise from 14.00°C to 39.98°C over a time of 14.9 minutes. Next, 5.570g 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 60.18°C . Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. →+2C2H2g 5O2g + 4CO2g 2H2Og Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students:…
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). First, a 5.500 g tablet of benzoic acid (C6H5CO₂H) 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 48.06 °C over a time of 5.8 minutes. Next, 5.630 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 18.00 °C to 77.25 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: C₂H₁(g) + 302(g) - 200,(s) + 2H,O(g) n thermometer stirrer ☑ chemical reaction "bomb" A "bomb" calorimeter. water insulation Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for…
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…
The complete combustion of salicylic acid releases 21.90 kJ of energy per gram of salicylic acid.In a particular bomb calorimeter (initially at room temperature), the combustion of 0.2745 g of salicylic acid, in the presence of excess oxygen, causes the temperature of the calorimeter to rise by 1.85 °C.When a 0.2999-g sample of an unknown organic substance is similarly burned in the same calorimeter, the temperature rises by 3.59 °C.What is the energy of combustion per unit mass of the unknown substance?
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…
When 6.10 g of urea,(NH2)2CO (g), burns to produce CO2 (g), N2 (g) and H2O (l) 67.8 kJ of heat energy are released in a bomb calorimeter. What is the energy released in the burning of one mole of urea? Using this, what is the enthalpy of formation of urea?
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…
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). thermometer stirrer First, a 5.500 g tablet of benzoic acid (C,H,CO, H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed insulation to rise from 15.00 °C to 42.56 °C over a time of 10.3 minutes. Next, 5.720 g of acetaldehyde (C2H,O} 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 40.53 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,0(g) + 50, (g) 4CO, (g) + 4H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note…
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.…
2 C,H,0(g) + 50,(8) 4 CO2(g) + 4 H,0(g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match published values for this reaction. exothermic Is this reaction exothermic, endothermic, or neither? endothermic O 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. kJ kJ Calculate the reaction enthalpy AH, per mole of C,H¸0. rxn mol