Calculate AHrxn for the reaction below.2 NOCI(g) → N2(g) + 02(g) + Cl2(9)You are given the following set of reactions.1/2 N2(g) + 1/2 02(g) → NO(g)AH = 90.30 k)NO(g) + 1/2 Cl2(g) → NOCI(g)AH = -38.6 kJ4.0kJ

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Answered: Calculate AHpxn for the reaction below.…

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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Given the reactions, X(s) + O₂(g) — XO(s) XCO3(s) what is AH for this reaction? X(s) + 1/2O₂(g) + CO₂(g) AH = XO(s) + CO₂(g) AH = -545.7 kJ AH = +433.9 kJ XCO3(s) kJ
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.
For which of the following reactions is AS> 0. OH₂ CO(g) + O2(g) → CO2(g) + H2O(1) O2 CO2(g) + N2(g) 2 CO(g) + 2 NO(g) OH2(g) + C2H4(g) →C2H6(g) ONH4 Cl(s) → NH3(g) + HCl(g) OCH4(g) + H2O(g) →3H2(g) + CO(g)
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The sun supplies energy at a rate of about 1.0 kilowatt per square meter of surface area (1 watt = 1 J/s). The plants in an agricultural field produce the equivalent of 23 kg of sucrose (C12H22 O11) per hour per hectare (1 ha = 10,000 m²). Assuming that sucrose is produced by the reaction 12CO₂(g) + 11H₂O(l) → C12H22 O11 (8) + 1202 (9) AH = 5640 kJ calculate the percentage of sunlight used to produce the sucrose - that is, determine the efficiency of photosynthesis in this field. Percent efficiency = %
When 130. mL of 0.198 M NaCl(aq) and 130. mL of 0.198 M AgNO3(aq), both at 21.8°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 24.2°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 2.60 ✕ 103 J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g·°C, and 0.997 g/mL, respectively). Using this data, calculate ΔH in kJ/mol of AgNO3(aq) for the given reaction. This is the complete question, nothing was left out. Thank you
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1. What is the final overall reaction for these three reactions below? Reaction 1: C3 Hs (g) + 5 O2 (g) → 3 CO2 (g) +4 H2O (g), AH1 = -2043 kJ Reaction 2: C (s) + O2 (g) Reaction 3: 2 H2 (g) + O2 (g) + CO2 (g), AH2 = -393.5 kJ 2 H2O (g), AH3 -483.6 kJ Hint. Reverse Reaction 1 then simplify by cancelling compounds in opposite sides of the arrow.
21
Given the following equation: 2H3PO4 + 3Mg(OH)2 → 6 H2O + Ca3(PO4)2 + 450.8 kJ If 300 mL of 0.75 mols/L phosphoric acid solution, H3PO4, is mixed with 25.0 g of magnesium hydroxide, Mg(OH)2, predict the amount of energy released Note: the sign (-/+) is not relevant to the question. Your answer should follow the format: a) mols of H3PO4 b) maximum energy released if all of the H3PO4 reacts (with units) c) mols of Mg(OH)2 d) maximum energy released if all of the Mg(OH)2 reacts (with units) e) based on your answer to (b) and (d), how much energy will be released by this reaction based on the quantities of reactants indicated.

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Calculate AHpxn for the reaction below. 2 NOCI(g) → N2(g) + O2(g) + Cl2(g) You are given the following set of reactions. 1/2 N2(g) + 1/2 02(9) → NO(9) AH = 90.30 k) NO(g) + 1/2 Cl2(g) → NOCI(g) AH = -38.6 k) 4.0 kJ