Nitrogen dioxide, NO2, an air pollutant, dissolves in rainwater to form a dilute solution of nitric acid. The equation for the reaction 3NO2 (g) + H2O (L) - - - > 2HNO3 (L) + NO CALCULATE THE change of S0 FOR THIS REACTION IN J/K

Nitrogen dioxide, NO2, an air pollutant, dissolves in rainwater to form a dilute solution of nitric acid. The equation for the reaction 3NO2 (g) + H2O (L) - - - > 2HNO3 (L) + NO CALCULATE THE change of S0 FOR THIS REACTION IN J/K

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

See similar textbooks

Related questions

Q: 9. Calculate AH for the following reaction: 2B (s)+ 3,0,(g) → B,0, (s) Use the following reactions…

A: Answer:

Q: Nitrogen oxides undergo many interesting reactions in the environment and in industry. Given the…

A: The enthalpy change for the overall equation is - 109.5 KJ.

Q: Calculate ΔG°rxn (in kJ) for a reaction where ΔH°= +63 kJ, ΔS°= +675 J/K, and T = 298 K

Q: There are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of…

A: Calcium carbide is widely used in the industrial preparation of acrylic acid.

Q: Under the standard state and 260 °C, the solid of ammonia hydroxide NH4OH (s) decomposes explosively…

A: NH4OH (s) ==> NH3 (g) + H2O (g)

Q: Consider the following balanced chemical equation for the combustion of acetylene (CH): Overall…

A: Hess's law is used here. According to Hess's law, the overall enthalpy of the reaction is the sum of…

Q: Calculate AH° for the reaction: Na,0(s) + SO;(g) – Na,SO,(g) given the following information: AH°…

Q: Be sure to answer all parts. Deterioration of buildings, bridges, and other structures through the…

A: The balance chemical equation for rusting of iron is as follow 4Fe(s)…

Q: 73. Given the following data Ca(s) + 2C(graphite) → CaC2(s) Ca(s) + O,(g) –→ CaO(s) CaO(s) + H,O(1)…

Q: Calculate the ΔSsurr in kJ/K for the following reaction at 50°C. 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6…

Q: 5.00 g of potassium hydroxide (molar mass = 56.1 g/mol) dissolves in 100.0 g of water and the…

A: The information given in the question is as follows: Mass of potassium hydroxide = 5.00 g Molar mass…

Q: A solid 30.2 cm^3 block of KClO3 is heated in the laboratory and decomposes according to the…

Q: Chemists have been performing experiments with the newly discovered element X to determine its…

A: The reaction given is And ΔHo for the reaction = -191 KJ Given : Under standard conditions, X is…

Q: Consider the decomposition of liquid benzene, C6H6(l), togaseous acetylene, C2H2(g):C6H6(l)…

A: a) C6H6(l) -----> 3 C2H2(g) ΔH = +630 kJ the enthalpy change for the reverse reaction 3 C2H2(g)…

Q: 63. Calculate ΔH°ΔH° for the process Sb(s)+5/2Cl2(g)⟶SbCl5(s) from the following…

A: The required reaction is: The given reactions are:

Q: 1. 1. Zinc metal reacts with HCl according to the following equation: Znw + HClag) → ZnClz{aq) +…

A: The formula for density is, Rearranging it to calculate the mass from volume and the density of…

Q: Q2.) For a particular reaction, ΔH = -32 kJ and ΔS = -90 J/K . Assume that ΔH and ΔS do not vary…

A: Given : ΔH = -32 kJ ΔS = -90 J/K 1) To calculate Temperature at which ΔG=0 ΔG = ΔH - TΔS ΔG=0…

Q: The dissolution of ammonium nitrate occurs spontaneously in water. As NH4NO3 dissolves, the…

Q: The value of AH° for the reaction below is -126 k). The amount of heat that is released by the…

A: Sodium peroxide reacts with water to form sodium hydroxide and oxygen. The equation for the balanced…

Q: Hydrogen peroxide (H2O2) decomposes to water and oxygen at constant pressure by the following…

A: Since from the given reaction we can say that when 2 moles (2 because in reaction coefficient of…

Q: When a 25.0 g sample of AgNO3 dissolves in 100.0 g of water in a calorimeter, the temperature drops…

A: The change in enthalpy (∆H) of a reaction is given by the equation: ∆H = m×C×∆T ⋯⋯⋯⋯⋯⋯(1) where m is…

Q: CaO(s) + Cl2(g) ⟶ CaOCl2(s) ΔH = -110.9kJ H2O(l) + CaOCl2(s) + 2NaBr(s) ⟶…

Q: The fat, glyceryl trioleate (C57H10406), is metabolized via the following reaction. Given the…

Q: Silver carbonate, Ag, CO3, is a light yellow compound that decomposes when heated to give silver…

A: To calculate partial pressure of carbon dioxide:

Q: Given the data in the table below, calculate AH° (kJ) for the reaction: 2CH3OH) + 302G) - 2C029) +…

A: Given,

Q: 4. Find the standard molar enthalpy for the reaction C(s) + % O2(g) – CO(g) C(s) + 02(g) – cOo2(g)…

A: The enthalpy of the reaction is considered as the state function that is it depends only on the…

Q: Using Hess's Law tó calculate net reaction enthalpy 1/5 The lead-acid storage battery is the oldest…

Q: a solid 30.2 cm³ block of KClO₃ is heated in the laboratory and decomposes according to the…

Q: The overall reaction in a commercial heat pack can be represented as 4 Fe(s) +302 (9)→ 2 Fe,O,(s) AH…

A: Heat capacity of a substance or system indicates the amount of heat required to raise the…

Q: Consider the following generic chemical equation whose ΔHrxn is unknown. Target: 2A+7B⟶4X Instead,…

Q: Calculate AG°rxn (in kJ) for a reaction where AH°= +124 kJ, AS°= +223 J/K, and T = 298 K %3D

A: Given; Enthalpy of the reaction (∆H°) = + 124 kJ Entropy of the reaction (∆S°) = + 223 J/K = + 0.223…

Q: A chemist measures the enthalpy change AH during the following reaction: 8 SO,(g) + 16 H, S(9)→3…

A: Here by applying Hess Law ,we can determine the enthalpy of reactions of different form of a…

Q: 5. Calculate and draw the enthalpy diagram for the following reaction: Mg(s) + H 20(g) –→ Mg0(s) +…

A: Enthalpy diagram : An enthalpy diagram plots potential energy on the Y-axis and reaction progress on…

Q: Hemoglobin carries O₂ from the lungs to tissue cells, wherethe O₂ is released. The protein is…

Q: Given the following chemical reaction occurring in a 2.00 L container: A (g) + 2 B(s) ↔ 4 C(g) + 3…

Q: 5. Calculate the value of ΔSo for the formation of calcium chloride from its constituent elements,…

Q: 1. Iron(II) oxide (FeO) is used in cosmetics and in tattoo inks as a dye. Iron(II) oxide reacts with…

Q: Calculate the AHn for the formation of 1 mole of PbOs) from lead metal and oxygen gas, given the…

Q: . Calculate ΔH° for the process Co3 O4(s) ⟶ 3Co(s) + 2O 2(g) from the following information:

A: The above problem is based on Hess's law, The enthalpy change for the overall process is the sum of…

Q: CaCOg(s) -> CaO(s) +CO2 AH=177.8 kJ/mol What is the change in the internal energy for the reaction…

Q: Predict the sign, + − or 0, of ASº for each of the following reactions a) Oxygen gas and nitrogen…

Q: Calculate the enthalpy for the decomposition of calcium carbonate according to the equation CaCO3(s)…

A: Enthalpy for decomposition of calcium carbonate is calculated by using Hess's law.

Q: the laboratory, POCl3 (phosphorus oxychloride) is used in the manufacture of phosphate esters, which…

Q: 20) Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction:…

Q: Given the following equation, N20(g) + NO28) → 3 NO(g) AG°rxn = -23.0 kJ Calculate AG° rxn for the…

A: When a thermochemical equation is multiplied with a number then its ∆H° or ∆G° value also gets…

Q: Consider the decomposition of liquid benzene, C6H6(l), to gaseous acetylene, C2H2(g): ⅓C6H6(l) --->…

Q: For the reaction 2 A(g) → A2(g), Q = -20.00 kJ for the formation of one mole of A2(g) at constant…

A: Given data: The reaction is- 2 A(g) → A2(g), Q = -20.00 kJ Temperature = 25.00◦C

Q: In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon…

Q: 2. For the following reaction at 25°C, AG° is -118.4 kJ. At what pressure of O2 gas does AG = 0 at…

Q: The dissolution of ammonium nitrate occurs spontaneously in water. As NH4NO3 dissolves, the…

A: According to the second law of thermodynamics, the spontaneous nature of the reaction is determined…

Question

Nitrogen dioxide, NO2, an air pollutant, dissolves in rainwater to form a dilute solution of nitric acid. The equation for the reaction

3NO2 (g) + H2O (L) - - - > 2HNO3 (L) + NO

CALCULATE THE change of S⁰ FOR THIS REACTION IN J/K

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

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup calorimeter. As Ag2O(s) precipitates, the temperature of the solution increases from 23.78 C to 25.19 C. Assuming that the mixture has the same specific heat as water and a mass of 150 g, calculate the heat q. Is the precipitation reaction exothermic or endothermic?
A student performing a calorimetry experiment combined 100.0 ml. of 0.50 M HCI and 100.0 ml. of 0.50 M NaOH in a StyrofoamTM cup calorimeter. Both solutions were initially at 20.0 C, but when the two were mixed, the temperature rose to 23.2 C (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 ml of 0.50 M NaOH. WIII the AT observed be greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCI and 100.0 ml. of 1.00 M NaOH. Will the T observed be greater than, less than, or equal to that in the first experiment, and why?
When 50.0 g of 0.200 M NaCl(aq) at 24.1 C is added to 100.0 g of 0.100 M AgNO3(aq) at 24.1 C in a calorimeter, the temperature increases to 25.2 C as AgCl(s) forms. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat in joules produced.
A 250-g sample of water at 20.0C is placed in a freezer that is held at a constant temperature of 20.0C. Considering the water as the system, answer the following questions: a What is the sign of qsys for the water after it is placed in the freezer? b After a few hours, what will be the state of the water? c How will the initial enthalpy for the water compare with the final enthalpy of the water after it has spent several hours in the freezer? d What will the temperature of the water be after several hours in the freezer?
In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both solutions were originally at 24.6C. After the reaction, the final temperature is 31.3C. Assuming that all the solutions have a density of 1.0 g/cm3 and a specific heat capacity of 4.18 J/Cg, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.
Peanuts and peanut oil are organic materials and bum in air. How many burning peanuts does it take to provide the energy to boil a cup of water (250 mL of water)? To solve this problem, we assume each peanut, with an average mass of 0.73 g, is 49% peanut oil and 21% starch; the remainder is noncombustible We further assume peanut oil is palmitic acid, C16H32O2, with an enthalpy of formation of 848.4 kJ/mol. Starch is a long chain of C6H10O5 units, each unit having an enthalpy of formation of 960 kJ.
9.53 Using these reactions, find the standard enthalpy change for the formation of 1 mol of PhO(s) from lead metal and oxygen gas. PbO(s)+C(graphite)Pb(s)+CO(g) H = 106.8 kJ 2C(graphite)+O2(g)2CO(g) H= -221.0 kJ If 250 g of lead reacts with oxygen to form lead(II) oxide, what quantity of thermal energy (in kJ) is ahsorhed or evolved?
Consider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(OH)2 Assuming that the temperature of both solutions was initially 25.0C and that the final mixture has a mass of 400.0 g and a specific heat capacity of 4.18 J/C g, calculate the final temperature of the mixture.
A volume of 1.50 L of argon gas is confined in a cylinder with a movable piston under a constant pressure of 1.22 105 Pa. When 1.25 kJ of energy in the form of heat is transferred from the surroundings to the gas, the internal energy of the gas increases by 1.11 kJ. What is the final volume of argon gas in the cylinder?
A 5.00-g sample of aluminum pellets (specific heat capacity = 0.89 J/C g) and a 10.00-g sample of iron pellets (specific heat capacity = 0.45 J/C g) are heated to 100.0C. The mixture of hot iron and aluminum is then dropped into 97.3 g water at 22.0C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings.
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
Combustion of table sugar produces CO2(g) and H2O( l). When 1.46 g table sugar is combusted in a constant-volume (bomb) calorimeter, 24.00 kJ of heat is liberated. a. Assuming that table sugar is pure sucrose, C12H22O11 (s), write the balanced equation for the combustion reaction. b. Calculate E in kJ/mol C12H22O11 for the combustion reaction of sucrose.