1.Based on the reactions:1. 2NO2 (g)→N204 (2)AHj = - 57.2 kJ2. 2NOg) + 02 g)→2NO2 ) A H2 = -114.1 kJUse Hess's law to calculate H for:2NO2 + 02 (g)→N,O4 (g) AH=|kJ

By Hess's law : Required equation = equn 1 + equn 2 ∆H = ∆H1 + ∆H2 = -57.2 + ( -114.1 )…

Answered: Based on the reactions: 1. 2NO2…

Based on the reactions: 1. 2NO2 (2)→N204 (g) AH1 =- 57.2 kJ 2. 2NOg) + 02 (g)→2NO2 (2) AH2 = -114.1 kJ Use Hess's law to calculate H for: 2NO g) ,+02 ()→N,04 (g) AH=| kJ

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.75E: Draw a diagram like Figure 2.11 that illustrates the change in enthalpy for the chemical reaction C...

See similar textbooks

Related questions

Q: For the chemical reaction Ca (s) + ½ O₂ (g) → CaO (s) ∆H° = -635 kJ/mol. What is the molar enthalpy…

A: The balanced Chemical equation given in the question - Ca(s) + ½O₂(g) → CaO(s), ∆H° =-635 kJ/mol…

Q: The standard enthalpy values, Δ?∘ , for several reactions are given. H2(g)+12O2(g)⟶H2O(l)Δ?∘=−286…

Q: Given the standard enthalpy changes for the following two reactions (1) 4C(s) + 5H2(g)–C,H10(g) AH°…

A: If the given reaction is multiplied by 2 by two, then value of the given standard enthalpy change…

Q: The molar heat capacity at constant pressure for CO(g) is 6.97 cal mol-1 K-1. How much heat in cal…

A: Data given: The molar heat capacity at constant pressure for CO(g), cp = 6.97 cal mol-1 K-1 Mass of…

Q: A reaction of 1.00 gram of NaOH with 100 mL of 1.0 M HCl in a styrofoam calorimeter causes a 10.5°C…

A: The mass (m) of the reaction solution is calculated as shown below where 100 mL is the total volume…

Q: The white pigment TiO2 is prepared by the reaction of titanium tetrachloride, TiCl4, with water…

Q: In a constant‑pressure calorimeter, 70.0 mL of 0.850 M H2SO4 was added to 70.0 mL of 0.270 M NaOH.…

A: The reaction taking place between H2SO4 and NaOH is as follows:

Q: 4. Consider the following equations: 4 PCI; 1. P₁ + 6 Cl₂ → P₁ +50₂ → 2. P₂010 AH₁ = -1226 kJ AH₂ =…

A: Given, Enthalpy change for the few reactions are given, 1) P4 + 6Cl2 ➝ 4PCl3 ∆H1 = -1226 kJ 2) P4 +…

Q: Using the equations 2 H2 (g) + O2 (g) → 2 H¿0 (I) AH° = -572 kJ/mol Ca (s) + ½ O2 (g) → CaO (s) AH°…

A: If we multiply by any number or divide to the chemical reaction then ∆H will also multiply or divide…

Q: Using the equations 2 H2 (g) + O2 (g) → 2 H2O (1) AH° = -572 kJ/mol Ca (s) + ½ O2 (g) → CaO (s) AH°…

Q: 11-12. The same quantity of energy is added to 25.0 g pieces of gold (molar heat capacity = 25.41…

A: Given data,Mass of Au=25gMass of Mg=25gMass of…

Q: Use the standard reaction enthalpies given below to determine ΔH°rxnfor the following reaction:…

Q: what is the change in the enthalpy in kj/kg for the complete combustion of 39.0 g of fructose,…

Q: (1) N2(g) + 202(g)→2NO2(g) AH° = 66.4 kJ (2) 2N½0(g)2N2(g) + O2(g) AH° = -164.2 kJ what is the…

A: Given, N2(g)+2O2(g)→2NO2(g) ∆Ho=66.4kJ--------(1)2N2O(g)→2N2(g)+O2(g) ∆Ho=-164.2kJ--------(2)

Q: Nitrogen and oxygen gas combine to form nitrogen dioxide according to the reaction N2(g) + 20s(g)…

Q: 3. The production of steel from iron involves the removal of many impurities in the iron ore. The…

A: All elements in their standard states (oxygen gas, solid carbon in the form of graphite, etc.) have…

Q: A calorimeter contains 130 g water. The calorimeter and the water inside are both at 26 °C. A piece…

A: Specific heat capacity of metal can be determined by calculating the heat loss by metal which is…

Q: For a certain chemical reaction, the AH of enthalpy is 232.4 kJ per one mole of reactant X. If 3 mol…

A: Enthalpy is the heat content of the system. For a reaction,change is energy is called enthalpy of…

Q: The enthalpy for the formation of 1 mole of NH3(aq) is -80.29 kJ/mol. What is the enthapy for the…

A: The heat of formation of a compound is defined as the heat change accompanying for the formation of…

Q: When 150 mL of 1.00 M NaOH is added to 100 mL of 1.30 M HCl in an insulated calorimeter, the…

A: To calculate the enthalpy change for the neutralization reaction, the following quantities are…

Q: Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 20.9 g…

A: Given data : Molar mass of KNO3 (MK)= 101.1 g/mol Mass of KNO3 (mK) = 20.9 g Mass of water (mw) =…

Q: 1. When 2.00 grams of solid sodium hydroxide dissolves in 100.0 ml of water in a coffee-cup…

Q: 1. 6FEO + 02 g) →2F@;O4 (6) 2Fe304 (3) AH=-3607.2 kJ 2. 4Fe;O4 (3) + 02 (3)→6FE;O3 (5) AH2 = +3408 3…

A: Introduction: Hess’s law states that enthalpy is a state function according to this law when a…

Q: Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 34.4 g…

A: Given that: Mass of KNO3 = 34.4 g, mass of water = 217 g, initial temperature of water, Ti = 23.00⁰C…

Q: Si(s) + 2 F2(g) ΔH° = 1.61×103 kJ What is the standard enthalpy change for this reaction…

Q: What mass of aluminum metal would absorb 250.0 kJ when it melted at its melting point? The molar…

A: One gram of aluminium metal absorbs 396.6 Joule heat.

Q: Using the equations 2 H2 (g) + O2 (g) → 2 H2O (I) AH° = -572 kJ/mol Ca (s) + ½ O2 (g) → CaO (s) AH°…

Q: Which of the following energy quantities is equivalent to 258 Cal? A. 258 cal B.1080 J C.…

A: 1 cal=4.184 joules

Q: A bomb calorimetry experiment is performed with xylose, C5H10O5(s) (molar mass = 150.13 g/mol), as…

Q: The following two reactions are known: N2(g) + O2(g) -> 2NO(g) AH = +180.50 kJ N2(g) + 202(g) ---> A…

Q: The molar heat capacity at constant pressure for CO(g) is 6.97 cal mol-1 K-1. How much heat in cal…

Q: Hydrobromic acid (HBr) is a commonly used acid for adding bromine to organic compounds. As bromine…

Q: Calculate the change in internal energy (ΔU) for a system that is giving off 25.0 kJ of heat and is…

A: The first law of thermodynamics states that the change in internal energy of a system equals the net…

Q: Using the equations 2 Fe (s) + 3 Cl, (g) → 2 FeCl, (s) AH° = -800.0 kJ/mol Si(s) + 2 CI, (g) → SICI,…

Q: Using the equations Ca (s) + ½ O2 (g) → CaO (s) AH° = -635 kJ/mol CaO (s) + H2O (1) → Ca(OH)2 (s)…

A: Let Ca (s) + 1/2 O2 (g) → CaO (s) ΔHo = -635 kJ/mol this be equation 1CaO (s) + H2O (l) → Ca(OH)2…

Q: Consider the following thermochemical data: Cl2(g) → 2CI(g) AH° = 242.3 kJ l2(g) → 21(g) AH° = 151.0…

Q: When 18.5 g of HgO(s) is decomposed to form Hg(l) and O2(g), 7.75 kJ of heat is absorbed at…

A: From standard sources, we get:- Molar mass of HgO = 216.59 g/mol Amount of HgO consumed = 18.5g

Q: Benzoic acid is used to determine the heat capacity of bomb calorimeters because it can be obtained…

A: Given that : The energy of combustion (Hcombustion) = -26.43 kJ/g Temperature increase (∆T) =…

Q: Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H2(g)→C„H1(g) AH°…

A: ∆H° is negative means that it is e reaction To get equation 3 we should multiply equation 2 by 2…

Q: For the chemical reaction H2 (g) + F2 (g) → 2 HF (g) AH° = -79.2 kJ/mol. What is the molar enthalpy…

Q: The reaction of 1.00 mol of solid phosphorus with chlorine gas to form PCl3(g) releases 287.0kJ of…

A: According to the Hess's law, the total change in enthalpy during a course of a chemical reaction…

Q: Given the following data: 2NO(g), N2(g) + 2NO(g) + O2 (g) → O2 (g) → 2NO2(g), 2N2O(g) → ΔΗ 180.7 kJ…

A: The answer is given as follows

Q: The heat capacity of silicon dioxide (SiO2, 60.1 g mol-1), is 0.732 J g¬ K-1. Calculate the energy…

A: The heat capacity of SiO2 is = 0.732 J g-1 K-1 The molar mass of SiO2 is =60.1 g.mol-1 The moles of…

Q: 10.0 mol CsH20, (glucose) is combusted to carbon dioxide and water at 25C according to the equation:…

Q: NO3KNO3 is dissolved in 229 g of water at 23.00 °C. KNO3(s)−→−−H2OK+(aq)+NO−3(aq) The…

Q: Consider the following reaction: N2(g) + 3H2(g) - 2NH3(g); AH° = - 91.8 kJ The density of ammonia at…

A: Calculate the mass of nitrogen gas. Mass of nitrogen gas = Volume of nitrogen gas × Density of…

Q: Given the standard enthalpy changes for the following two reactions: (1) N2(g) + 202(g)N½O4(g) AH° =…

A: You have given a reaction that follows the Hess Law of enthalpy formation.

Q: Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 48.7 g…

Question

1.
Based on the reactions:
1. 2NO2 (g)→N204 (2)
AHj = - 57.2 kJ
2. 2NOg) + 02 g)→2NO2 ) A H2 = -114.1 kJ
Use Hess's law to calculate H for:
2NO2 + 02 (g)→N,O4 (g) AH=|
kJ

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps

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

The enthalpy of combustion of hard coal averages 35 kJ/g, that of gasoline, 1.28105 kJ/gal. How many kilograms of hard coal provide the same amount of heat as is available from 1.0 gallon of gasoline? Assume that the density of gasoline is 0.692 g/mL (the same as the density of isooctane).
n Section 10.7, two characteristics of enthalpy changes for reactions are listed. What are these characteristics? Explain why these characteristics are true.
The enthalpy change when 1 mol methane (CH4) is burned is 890 kJ. It takes 44.0 kJ to vaporize 1 mol water. What mass of methane must be burned to provide the heat needed to vaporize 1.00 g water?
The thermochemical equation for the burning of methane, the main component of natural gas, is CH4(g)+2O2(g)CO2(g)+2H2O(l)H=890kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = 890 kJ? (c) What is the enthalpy change when 1.00 g methane burns in an excess of oxygen?
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
Dissolving 6.00 g CaCl2 in 300 mL of water causes the temperature of the solution to increase by 3.43 C. Assume that the specific heat of the solution is 4.18 J/g K and its mass is 306 g. (a) Calculate the enthalpy change when the CaCl2 dissolves. Is the process exothermic or endothermic? (b) Determine H on a molar basis for CaCl2(s)H2OCa2+(aq)+2Cl(aq)
The enthalpy changes for the following reactions can be measured: CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g) rH = 802.4 kJ/mol-rxn CH3OH(g) + 32 O2(g) CO2(g) + 2 H2O(g) rH = 676 kJ/mol-rxn (a) Use these values and Hesss law to determine the enthalpy change for the reaction CH4(g) + O2(g) CH3OH(g) (b) Draw an energy level diagram that shows the relationship between the energy quantities involved in this problem.
The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
In a coffee-cup calorimeter, 150.0 mL of 0.50 M HCI is added to 50.0 mL of 1.00 M NaOH to make 200.0 g solution at an initial temperature of 48.2C. If the enthalpy of neutralization for the reaction between a strong acid and a strong base is 56 kJ/mol, calculate the final temperature of the calorimeter contents. Assume the specific heat capacity of the solution is 4.184 J/g C and assume no heat Joss to the surroundings.
Calculate H for the reaction N2H4(l)+O2(g)N2(g)+2H2O(l) given the following data: Equation H(KJ) 2NH3(g)+3N2O(g)4N2(g)+3H2O(l) 1010 N2O(g)+3H2(g)N2H4(l)+H2O(l) 317 2NH3(g)+12O2(g)N2H4(l)+H2O(l) 143 H2(g)+12O2(g)H2O(l) 286
Given: 2Cu2O(s) + O2(g) 4CuO(s)H = 288 kJ Cu2O(s) CuO(s) + CuO(s)H = 11kJ Calculate the standard enthalpy of formation (Ht) for CuO(s).
Camping stoves are fueled by propane (C3H8), butane [C4H10(g), fH = 127.1 kJ/mol]. gasoline. or ethanol (C2H5OH). Calculate the enthalpy of combustion per gram of each of these fuels. [Assume that gasoline is represented by isooctane, C8H18(), with fH = 259.3 kJ/mol.) Do you notice any great differences among these fuels? How are these differences related to their composition?