A sample of solid benzoic acid (C,H;COOH) that weighs 800 g is burned in an excess of oxygen to CO,(g) and H,O(€) in a constant-volume calorimeter at 25°C. The temperature increase is observed to be 2.15°C. The heat capacity of the calorimeter and its contents is known to be 9382 J K-1. (a) Write and balance the equation for the combustion of benzoic acid. (b) Calculate the standard change in internal energy (AU°) for the combustion of 1.000 mol benzoic acid to CO2(g) and H,O(€) at 25°C. lc) Calculate the standard enthalpy change (AH°) for the same reaction as in part (b). (d) Calculate the standard enthalpy of formation per mole of benzoic acid, using data for the standard enthalpies of formation of CO2(g) and H,O(() from Appendix D.

A sample of solid benzoic acid (C,H;COOH) that weighs 800 g is burned in an excess of oxygen to CO,(g) and H,O(€) in a constant-volume calorimeter at 25°C. The temperature increase is observed to be 2.15°C. The heat capacity of the calorimeter and its contents is known to be 9382 J K-1. (a) Write and balance the equation for the combustion of benzoic acid. (b) Calculate the standard change in internal energy (AU°) for the combustion of 1.000 mol benzoic acid to CO2(g) and H,O(€) at 25°C. lc) Calculate the standard enthalpy change (AH°) for the same reaction as in part (b). (d) Calculate the standard enthalpy of formation per mole of benzoic acid, using data for the standard enthalpies of formation of CO2(g) and H,O(() from Appendix D.

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: A sample of solid biphenyl weighing 0.5260 g was ignited in a bomb calorimeter initially at 25 °C,…

A: “Since you have posted multiple questions, we will provide the solution only to the first question…

Q: A sample of solid biphenyl weighing 0.5260 g was ignited in a bomb calorimeter initially at 25 °C,…

A: A) Mass of Benzoic acid, C6H5COOH = 0.7750 g Temperature rise = ∆T = 1.940 K Heat of combustion of…

Q: A 104.2 mL sample of 1.00 M NaOH is mixed with 52.1 ml of 1.00 MH2SO, in a large Styrofoam coffee…

A: Please find below the reaction taking place 2 NaOH (aq) + H2SO4 (aq) -----> Na2SO4 (aq) + 2 H2O…

Q: A styrofoam calorimeter contains 60.0 mL of 0.750 M H3C6H5O7 at 22.8oC. When 9.83 g NaHCO3 is added…

A: Change in enthalpy i.e. ∆Hreaction can be calculated using the formula: ∆Hreaction=mC∆T where, m is…

Q: A 2.50 g sample of powdered zinc is added to 100.0 mL of a 2.00 M aqueous solution of hydrobromic…

Q: In the following experiment, a coffee-cup calorimeter containing 100.0 mL of H2O is used. The…

A: The mass of CaCl2 added to water is = 9.20 g The enthalpy of dissolution of CaCl2 is = -82.8 kJ/mol…

Q: 4.11 g of a solid (17.3 g moF') was dissolved in liquid water in a calorimeter with a calorimeter…

A: Mass of solid = 4.11 gMolar mass of solid = 17.3 g/molMoles of solid = Mass of solid Molar mass of…

Q: For a certain ideal gas, the increase of enthalpy is 34 Kcal when the pressure increases from 0.11…

A: GIVEN:- For a certain ideal gas, the increase of enthalpy is 34 Kcal when the pressure increases…

Q: When exactly one mole of chrysene, C₁8H12(s) is burned at 25°C in a bomb calorimeter, AE = -8942.6…

Q: 3.79 g of a gas (66.3 g mol-1) was dissolved in liquid water in a calorimeter with a calorimeter…

Q: Find A,U for the combustion of methanol (CH3 OH) to carbon dioxide and liquid water from the…

Q: The compound cyclohexanol, C6H₁2O, is a good fuel. It is a liquid at ordinary temperatures. When the…

A: Answer:here, ai are stoichiometric coefficients of products and reactants respectively.

Q: 4.0

A: We will. Calculate ∆H

Q: 21.7 g of a basic solution was mixed with 87.6 g of water in a calorimeter with a calorimeter…

Q: Given the following reaction enthalpies: P,(s) + 6 Cl,(g) → 4 PCI,(g) =-1225.6moi → PO,(s) → PCI,(g)…

Q: 5b. The Standard Molar Enthalpy of Formation (AH° f ) of hydrogen cyanide, (HCN(g)), cannot be…

Q: 22. Calculate the enthalpy change of formation of HNO, (aq) in the following reaction: Tultiple C…

Q: b) What is the standard enthalpy of reaction per mole of KOH when 50.00 cm³ of 1.0 moldm³ of Nitric…

A: Enthalpy of reaction: The Heat of Reaction (which is also known as the Enthalpy of Reaction)…

Q: Suppose 0.100 mol of a metal (M) is combusted in excess O2(g) in a bomb calorimeter. 4M(s) + 302…

A: Given: 4M + 3O2 -----> 2M2O

Q: A critical reaction in the production of energy to do work or drive chemical reactions in biological…

A: The given reaction is, ATPaq+H2Ol→ADPaq+HPO42-aq Also given, ∆Grxn°=-30.5 kJ/mol T=37°C=37+273=310K…

Q: Suppose 0.100 mol of a metal (M) is combusted in excess O2lg) in a bomb calorimeter. 4M(s) + 302 –…

A: Given the moles of metal, M that undergoes combustion = 0.100 mol the heat released during the…

Q: Calculate ΔHrxn

Q: Write the chemical equation for the standard molar enthalpy of formation of nitromethane, CH3NO2.

A: • We need to write the chemical equation for the standard molar enthalpy of formation of…

Q: 4.38 g of a gas (28.1 g mol–1) was dissolved in liquid water in a calorimeter with a calorimeter…

A: The question is based on the concept of chemical thermodynamics. We have to calculate enthalpy of…

Q: Calculate the change in internal energy (in kcal) for the reaction Cl2(g) + 7/2 O2(g) = Cl₂O7(g) at…

A: Given-> Cl2(g) + 7/2(O2) = Cl2O7(g) T = 25°C ∆H= 63.4 kcal/mole

Q: In Part B of the experiment, a student mixes 32.0 mL of 1.100 M HCl(aq) with 32.0 mL of 1.000 M…

A: Given,The volume of 1.100 M HCl= 32 mLThe volume of 1 M NaOH = 32 mLNote: 1mL = 10-3 LIncrease in…

Q: Determine, at 298 K, Ar1H°, the standard enthalpy of the reaction (1) between dinitrogen tetraoxide…

A: Welcome to bartleby !

Q: When 50.0 mL of 1.24 M of HCI(aq) is combined with 50.0 mL of 1.32 M of NaOH(aq) in a coffee-cup…

Q: A 2.50 g sample of powdered zinc is added to 100.0 mL of a 2.00 M aqueous solution of hydrobromic…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

A sample of solid benzoic acid (C,H;COOH) that weighs
800 g is burned in an excess of oxygen to CO,(g) and
H,O(€) in a constant-volume calorimeter at 25°C. The
temperature increase is observed to be 2.15°C. The heat
capacity of the calorimeter and its contents is known to be
9382 J K-1.
(a) Write and balance the equation for the combustion of
benzoic acid.
(b) Calculate the standard change in internal energy
(AU°) for the combustion of 1.000 mol benzoic acid
to CO2(g) and H,O(€) at 25°C.
lc) Calculate the standard enthalpy change (AH°) for the
same reaction as in part (b).
(d) Calculate the standard enthalpy of formation per
mole of benzoic acid, using data for the standard
enthalpies of formation of CO2(g) and H,O(() from
Appendix D.

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

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) b) What is the standard enthalpy of reaction per mole of KOH when 50.00 cm3 of 1.0 moldm-3 of Nitric Acid (HNO3) and 50.00 cm3 of 1.0 moldm-3 of Potassium Hydroxide (KOH) are mixed? According to your simulation, the temperature rose by __6.81__ oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1)
7. (a A 5.00 mol sample of an ideal gas is compressed irreversibly and isothermally at 150.00 K from an initial volume of 30.00 L in two steps: Step #1: Pext = 5.00 bar, Step #2: Pext = 20.00 bar. Determine the value of the total work and heat involved (in J). (b) Describe in words what happens to the total amount of work if the compression occurs in three steps. (c). Assuming the process could be done in one or multiple steps and the process could be reversible or irreversible, determine the minimum and maximum amount of work that could be done to complete the compression.
A sample of solid 9,10-phenanthrenediol (C14H1002) that weighs 0.6417 g is burned in an excess of oxygen to CO2(g) and H20(,) in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.140 °C. The heat capacity of the calorimeter and its contents is known to be 9.260x103 J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. 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 9,10-phenanthrenediol to CO2(g) and H20(,). kJ mol 1 1
a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) Show your working below:
A solution of 75.0 mL of 3.20 M HNO3 was mixed with 50.0 mL of 2.00 M Ca(OH)2 in a large Styrofoam coffee cup; the cup is fitted with a lid through which a calibrated thermometer passes. The temperature of both solutions before mixing was 20.1 °C. After the Ca(OH)2 solution is added to the coffee cup and the mixed solutions are stirred with the thermometer, the maximum temperature measured was 39.2 °C. Assume that the volumes are additive but that the density of the mixed solution is 1.10 g/mL, the specific heat of the mixed solution is 4.18 J/g•°C, and no heat is lost to the surroundings. In much the same way as you did for the previous question, calculate the enthalpy change per mole of HNO3 in the reaction. Consider that only reactants that actually react will account for the heat produced.
(2B) A heat engine operates between a hot source at 130.°C and a cold sink at 10.°C. How much workcan be done by the engine if 523 kJ of heat are extracted from the hot source?
CH,,0, (s) + 60, (g) → 6CO, (g) + 6H,0(g) 12 The combustion of glucose was performed in a bomb calorimeter. Qwater= 14.52kJ. The heat capacity of the bomb is Ca = 2.273 kJ/C and the change in temperature was 28.49C. If 0.03255 moles of glucose was used in the bomb calorimeter, then what is AHmy in kJ/mol? a. ´cal rnx
Q.30. Determine, at 298 K, Δr1H0, the standard enthalpy of the reaction (1) between dinitrogen tetraoxide and hydrazine: (1) N2O4 (g) + 2 N2H4 (l) à 3 N2 (g) + 4 H2O (g) Knowing the standard reaction enthalpies, at 298 K, of the following reactions: (2) NH3 (g)à 1/2 N2 (g) + 3/2 H2 (g) ; Δr2H0 = + 46,19 kJ . mol–1 (3) N2O4 (g) à 2 NO2 (g) ; Δr3H0 = + 58,04 kJ . mol–1 (4) 2 NH3 (g) à N2H (l) + H2 (g) ; Δr4H0 = + 142,80 kJ . mol–1 (5) 2 NO2 (g) + 4 H2 (g) à N2 (g) + 4 H2O (g) ; Δr5H0 = – 1 033,66 kJ . mol–1
4.00 g NaOH(s) (39.996 g mol–1) dissolves in 100.0 g of water in a constant–pressure calorimeter. The initial temperatures of both materials are the same at 20.0°C. The density of the solution is 1.00 g cm–3. The heat of dissolution is –44.51 kJ mol–1. The specific heat of the solution is 4.184 J g–1 °C–1. The specific heat of the calorimeter is 100 J °C–1. What is the final temperature of the solution? 30.23°C 25.94°C 28.32°C What is the energy lost to the calorimeter? 579 J 832 J 721 J