(Equation 1) 4 Fe2O3(s) + 20 NO2(g) + 22 H2O(l) + 5 O2(g) → 8 Fe(OH)3(s) + 20 HNO3(aq) AH= -1811.2 kJ/mol (Equation 2) Fe2O3(s) + 3 H2O (l) → 2 Fe(OH)3(s) AH = 35.6 kJ/mol (Equation 3) 20 HNO3(aq) → 5 O2(g) + 10 H2O (1) + 20 NO2(g) AH = ??????? The AH for equation 3 is: _________(express in kJ)

(Equation 1) 4 Fe2O3(s) + 20 NO2(g) + 22 H2O(l) + 5 O2(g) → 8 Fe(OH)3(s) + 20 HNO3(aq) AH= -1811.2 kJ/mol (Equation 2) Fe2O3(s) + 3 H2O (l) → 2 Fe(OH)3(s) AH = 35.6 kJ/mol (Equation 3) 20 HNO3(aq) → 5 O2(g) + 10 H2O (1) + 20 NO2(g) AH = ??????? The AH for equation 3 is: _________(express in kJ)

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...

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I am confused on how to find the enthalpy change with this information. Thank you!
Calculate AH for the following reaction, given the data in the table below: H2SO4(1) → SO3(g) + H2O(g) AH = ??? kJ/mol H2S(g) + 202(g) → H2SO4(1) AH = -698.0 kJ H2S(g) +202(g) → SO3{g) + H2O(1) AH = -203.0 kJ H2O(1) → H2O(g) AH = +29.32 kJ
You wish to find the enthalpy for the reaction 6 Gel4 (s) + 14 NH41 (s) → 3 Ge₂H6 (1) + 7 N₂ (g) + 38 HI (g) Given the following equations Equation 1: 2 Ge (s) + 3 H₂ (g) Ge₂H6 (1) AH = 137.3 kJ/mol Equation 2: Ge (s) + 4 HI (g) → Gel4 (s) + 2 H₂(g) AH = -247.8 kJ/mol Equation 3: 2 NH4I (s) → N₂ (g) + 2 HI (g) + 3 H₂(g) AH = 455.8 kJ/mol What would be the enthalpy change, in kJ/mol, for 6 Gel4 (s) + 12 H₂(g) → 6 Ge (s) + 24 HI (g)?
How do i combine these reactions for a combustion reaction?
Consider the following thermochemical equations (Note: HA is a weak acid)H+(aq) + OH-(aq) → H2O(l) ΔH1HA(aq) → H+(aq) + A-(aq) ΔH2HA(aq) + OH-(aq) → A-(aq) + H2O(l) ΔH3Choose the equation that shows the correct relationship between their enthalpy changes. A.) ΔH1 = ΔH3 - ΔH2 B.) ΔH2 = ΔH1 + ΔH3
A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 22.4 mL of 6.45 M hydrochloric acid. The temperature of the mixture rises 17.2 ° C. The density of the resulting solution is 1.00 g mL and has a specific heat capacity of 4.184 J g · ° C . The heat capacity of the calorimeter is 16.97 J ° C . Part 1: (a) Identify the limiting reagent for the reaction. Part 2: (b) Calculate the heat of reaction (in J). qrxn = × 10 JEnter your answer in scientific notation. Part 3 out of 3 (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization = ____ kj/mol
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Consider these reactions: Reaction 1: H₂(g) + Cl₂(g) → 2HCl(g) Reaction 2: 20F₂ (g) → O₂(g) + 2 F₂ (g) Reaction 3: N₂(g) + 2O₂(g) → 2NO₂ (9) Use Reaction 1. AH = -184.6 kJ AH = -49.4 kJ AH = +66.4 kJ Determine the mass, in grams, of chlorine gas consumed (with excess H₂) when 1,861.0 kJ of energy is released from the system. Round to the nearest whole number. Answer:____ g
Consider the following thermochemical equations (Note: HA is a weak acid)H+(aq) + OH-(aq) → H2O(l) ΔH1HA(aq) → H+(aq) + A-(aq) ΔH2HA(aq) + OH-(aq) → A-(aq) + H2O(l) ΔH3Choose the equation that shows the correct relationship between their enthalpy changes.
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