(Equation 1) 4 Fe2O3(s) + 20 NO2(g) + 22 H200) + 5 O2(g) → 8 Fe(OH)3(s) + 20 HNO3(ag) AH= -1811.2 kJ/mol (Equation 2) Fe203(s) + 3 H2Ou) → 2 Fe(OH)3(s) AH = 35.6 kJ/mol (Equation 3) 20 HNO3(ag)→ 5 O2(g) + 10 H2O1) + 20 NO2(g) AH = ??????? To find AH for equation 3 you must: Screen Reader Version Consider the problem below: (Equation 1) 4 "F"e2O3(s) + 20 NO2(g) + 22 H2O(1) + 5 O2(g) 8 "F"e left arrow parenthesis O H right parenthesis 3(s) + 20 HNO3(ag) AH= minus 1811.2 kJ/mol (Equation 2) F e2O3(s) + 3 H2O0) arrow 2 "F"e left parenthesis O H right parenthesis 3(s) AH = 35.6 kJ/mol (Equation 3) 20 HNO3(aq) arrow 5 O2(9) + 10 H2O1) + 20 NO2(g) AH = ??????? %3D To find AH for equation 3 you must: multiply equation 1 only multiply equation 2 only multiply equation 1 and equation 2 multiply neither equation 1 nor equation 2.

(Equation 1) 4 Fe2O3(s) + 20 NO2(g) + 22 H200) + 5 O2(g) → 8 Fe(OH)3(s) + 20 HNO3(ag) AH= -1811.2 kJ/mol (Equation 2) Fe203(s) + 3 H2Ou) → 2 Fe(OH)3(s) AH = 35.6 kJ/mol (Equation 3) 20 HNO3(ag)→ 5 O2(g) + 10 H2O1) + 20 NO2(g) AH = ??????? To find AH for equation 3 you must: Screen Reader Version Consider the problem below: (Equation 1) 4 "F"e2O3(s) + 20 NO2(g) + 22 H2O(1) + 5 O2(g) 8 "F"e left arrow parenthesis O H right parenthesis 3(s) + 20 HNO3(ag) AH= minus 1811.2 kJ/mol (Equation 2) F e2O3(s) + 3 H2O0) arrow 2 "F"e left parenthesis O H right parenthesis 3(s) AH = 35.6 kJ/mol (Equation 3) 20 HNO3(aq) arrow 5 O2(9) + 10 H2O1) + 20 NO2(g) AH = ??????? %3D To find AH for equation 3 you must: multiply equation 1 only multiply equation 2 only multiply equation 1 and equation 2 multiply neither equation 1 nor equation 2.

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

Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCI(aq) 2 MCI, (aq) + 3 H, (g) ΔΗ = -550.0 kJ 2. HCl(g) HCI(aq) AH2 = -74.8 kJ > 3. H, (g) + Cl, (g) → 2 HCl(g) AH3 = -1845.0 kJ 4. MCl, (s) → MCI, (aq) AH4 = -291.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) → 2 MCI, (s) ΔΗ kJ
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
Are the reactions endothermic or exothermic? What observation supports this?
50 g of solid sodium hydroxide is dissolved in 175 mL of water. Using a coffee-cup calorimeter, the temperature change of the water is measured to be -2.1°C. Which equation best describes this system? NaOH(s)→NaOH(aq) + kJ NaOH(s)+ kJ →NaOH(aq) NaOH(s)→NaOH(l) + kJ NaOH(aq)→NaOH(s) + kJ NaOH(aq)+ kJ →NaOH(s) NaOH(l)+ kJ → NaOH(s) What is the definition of the temperature of a substance? the speed of the slowest particles in the substance, subtracted from the speed of the fastest particles. the heat capacity of the substance times its mass a measure of the average kinetic energy of a system the total heat content of a substance the speed of the fastest particles in the substance Which statement describes an endothermic reaction? The surroundings warm up. The system releases energy. The potential energy of the products is less…
The addition of hydroiodic acid to a silver nitrate solution precipitates silver iodide according to the reaction: AGNO3 (aq) + HI(aq) → AgI(s) + HNO3 (aq) When 50.0 mL of 5.00x10-2 M AgNO3 is combined with 50.0 mL of 5.00x10-2 M HI in a coffee-cup calorimeter, the temperature changes from 22.40 °C to 22.91 °C. Part A Calculate AHrxn for the reaction as written. Use 1.00 g/mL as the density of the solution and Cs = 4.18 J/(g·°C) as the specific heat capacity of the solution. Express the energy to two significant figures and include the appropriate units. HẢ Units Value ΔΗΚΗ rxn
Which of the reactions are exothermic?
When octane (C8H18, density = 0.699 g/mL) undergoes complete combustion, it provides energy according to the reaction: 2C8H18(l)+25O2(g)→16CO2(g)+18H2O(l) ΔHo=−10,932kJ How much heat, in kJ, is produced by the amount of octane needed to drive 750 kilometers in a car that averages 20.1 km/L? ____ kJ
Consider the following chemical reaction which produces nitric oxide from its constituent elements: N2 (g) + O2(g) → 2 NO (g) AH = 182.6 kJ/mol If nitrogen and oxygen were mixed and allowed to react under constant pressure conditions, which of the following statements must be true? Select as many answers as applicable however points will be deducted for incorrect guesses. ΔΗ = q This is an endothermic reaction The temperature of the surroundings would decrease The temperature of the surroundings would increase AH = AU
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?
Consider these reactions: Reaction 1: H2(g) + Cl2(g) 2HCl(9) AH = -184.6 kJ Reaction 2: 20F2(g) → O2(g) +2F2(g) AH=-49.4 kJ Reaction 3: Na (g) +202 (9) 2NO2(g) AH = +66.4 kJ Use Reaction 1. Determine the mass, in grams, of chlorine gas consumed (with excess H₂) when 1,409.0 kJ of energy is released from the system. Round to the nearest whole number .
Given the standard enthalpy changes for the following two reactions: (1) 2Pb(s) + O₂(g) → 2PbO(s) (2) 2Zn(s) + O₂(g) → 2ZnO(s) Standard enthalpy change = AH-434.6 kJ AH° -696.6 kJ What is the standard enthalpy change for the following reaction? (3) PbO(s) + Zn(s) → Pb(s) + ZnO(s) AH° = ? KJ =
Using the equations - N₂(g) + O₂(g) → 2 NO (g) AH° = 180.6 kJ/mol N₂(g) + 3 H₂ (g) → 2 NH, (g) AH = -91.8 kJ/mol 2 H₂ (g) + O₂(g) → 2 H₂O (g) AH = -483.7 kJ/mol 2 Determine the molar enthalpy (in kJ/mol) for the reaction 4 NH, (g) + 5 O₂ (g) →4 NO (g) + 6 H₂O (g).