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

Related questions

Q: In an insulated bomb calorimeter, 0.568 g of solid citric acid (C6H8O7, molar mass 192.12 g) was…

Q: A student has a coffee-cup calorimeter with 50.0 g of water at 21.5oC. They introduce 15.525 g of…

A: The objective of the question is to find the final temperature of the magnesium metal in Kelvin…

Q: 3. 0.562 g of graphite is placed in a calorimeter with excess oxygen at 25.00 °C and 1 atm pressure.…

A: Mass of graphite = 0.562 g Molar mass = 12.01 g/mol Moles of graphite = MassMolar mass=0.562 g12.01…

Q: A 40.0 g sample of an unknown metal at 99.0 °C was placed in a constant-pressure calorimeter…

A: According to thermodynamics, the heat released by the hot metal equals the heat absorbed by the…

Q: If you said the reaction was exothermic or endothermic, calculate the amount of heat that was…

Q: When 0.525 g of toluene (C7H8) is combusted in a bomb calorimeter, thetemperature of the calorimeter…

A: First law of thermodynamics gives the relationship between the internal energy change (ΔErxn) and…

Q: When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution…

A: Given: Mass of Cs2SO4 = 22.75 gMass of water = 117.50 gInitial temperature = 25.42 °CFinal…

Q: Next, 4.490 g of ethylene (C₂H4) are put into the "bomb" and similarly completely burned in an…

Q: 4.900g of acetylene C2H2 are put into the "bomb" and similarly completely burned in an excess of…

A: Heat (q) gained or released is calculated using the following formula- q = m×C×∆T where m is the…

Q: A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water…

A: Step 1: Given:Mass of water = 1300 g.Initial temperature = 19.00 oC.Final temperature = 41.83…

Q: A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water…

A: C2H5OH + 3O2 = 2CO2 + 3H2O 1) The above reaction is…

Q: In an insulated bomb calorimeter, 0.568 g of solid citric acid (C6H&O7, molar mass 192.12 g) was…

Q: A chunk of titanium weighing 19.39 g and originally at 98.06 °C is carefully lowered into an…

A: Given data:Mass of titanium = 19.39 gInitial temperature of titanium = Mass of water = 81.56…

Q: A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water…

Q: A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of…

A: Calculate the number of moles of xanthone. nxanthone = WxanthoneMxanthonenxanthone = 0.517 g196…

Q: An electrical heater adds 21.9 kJ of heat to a constant-volume calorimeter. The temperature of the…

Q: A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water…

A: Given that: Mass of water = 1300 g Mass of benzoic acid = 5.500 g Temperature change for the…

Q: Use this information, and any other information you need from the ALEKS Data resource, to answer the…

A: Mass of water in bomb calorimeter=1200 gMass of ethylene=4.290 gMolar mass of ethylene=25…

Q: An electrical heater adds 23.7 kJ of heat to a constant - volume calorimeter. The temperature of the…

A: The objective of the question is to calculate the molar energy of combustion of methanol using the…

Q: In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used…

A: we have to calculate the final temperature

Q: Part A A 50.0-mL sample of a 1.00 M solution of is mixed with 50.0 mL of 2.00 M KOH in a…

Q: A student runs two experiments with a constant-volume "bomb" calorimeter containing 1400.g of water…

Q: A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water…

A: a.) Exothermic reaction is that reaction in which heat is released and endothermic reaction is that…

Q: 2. To study the possible amount of energy generated by a person, the person can be roughly viewed as…

Q: A chemical reaction is carried out in a calorimeter with the following heat capacity (C = 252.4…

A: The specific heat can be defined as the amount of heat per unit mass that is needed to raise the…

Q: A 307-g sample of an unknown mineral was heated to 98/1°C and placed into a calorimeter containing…

Q: Calculate the molar enthalpy for dissolving 25 g of NaCl in 100g of water inside a calorimeter. The…

A: Given: The mass of NaCl = 25 g The mass of water taken = 100 g The calorimeter heat capacity = 500…

Q: A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water…

A: Given that mass of water = 1200 g mass of benzoic acid = 7.000 gHeat of combustion of benzoic acid…

Q: A scientist measures the standard enthalpy change for the following reaction to be 6.7 kJ : CO(g) +…

Q: A scientist measures the standard enthalpy change for the following reaction to be 158.9 kJ:…

Q: A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water…

Question

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¯!

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Trending now

This is a popular solution!

Step by step

Solved in 6 steps with 6 images

SEE SOLUTION Check out a sample Q&A here

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