Page 1 of 2 Potential Energy (kJ) (i) Cl2 (g) + Pt (s) → 2Cl (g) + Pt (s) (ii) Cl (g)+ CO (g) + Pt (s) → CICO (g) + Pt (s) (iii) Cl (g)+CICO (g) → Cl₂CO (g) 1. Consider these three reactions as the elementary steps in the mechanism for a chemical reaction. 7 W Ea = 1550 kJ Ea = 2240 kJ Ea = 2350 kJ 2600 2400 2200 2000 1800 1600 1400 1200 1000 800 600 400 200 Q Search AH = -950 kJ ΔΗ = 575 kJ AH = -825 kJ a. Draw the potential energy diagram for the reaction. Label the data points for clarity. The potential energy of the reactants is 600 k

Page 1 of 2 Potential Energy (kJ) (i) Cl2 (g) + Pt (s) → 2Cl (g) + Pt (s) (ii) Cl (g)+ CO (g) + Pt (s) → CICO (g) + Pt (s) (iii) Cl (g)+CICO (g) → Cl₂CO (g) 1. Consider these three reactions as the elementary steps in the mechanism for a chemical reaction. 7 W Ea = 1550 kJ Ea = 2240 kJ Ea = 2350 kJ 2600 2400 2200 2000 1800 1600 1400 1200 1000 800 600 400 200 Q Search AH = -950 kJ ΔΗ = 575 kJ AH = -825 kJ a. Draw the potential energy diagram for the reaction. Label the data points for clarity. The potential energy of the reactants is 600 k

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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H2 (g) + Na (s) → F2 (g) + He (g) →
Cr(s) + O2(g)→ Cr,O3(s)
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Using the information below, calculate AH of NH3(g) + HCI(g) NH,CI(s). N, (8) + H, (8) NH,(g) AH = -46.19 kJ/mol > H, (g) + Cl,(8) → HCl(g) AH = -92.30 kJ/mol N, (8) + 2 H, (g) +Cl,(g) NH,Cl(s) AH = –314.4 kJ/mol • Your answer should have four significant figures. Provide your answer below: kJ/mol
How can the following reaction be rewritten to include the energy value within the chemical equation? Y2(g) + X2(g) ⟶ 2YX(g) ΔH = +90 kJ
(c) Using Hess Law and based on the equations, find enthalpy changes, AH, for this reaction;B N2H4() + H2(g) → 2NH3(g) AHr =? N2H4() +O2(g) → N2(g) + 2HO (g) AP = -543 kJ/mol 2H2(g) + O2(g) → 2H2O (g) AP =-484 kJ/mol N2(g) + 3H2(g) 2NH:(g) AP = -92.2 kJ/mol
a) In the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen gas. The thermodynamic equation for the reaction is HNO3(g) + 4H2(g) → NH3(g) + 3H2O(g) ΔH = –637 kJ Calculate the amount of energy released when one mole of hydrogen gas reacts. Consider this to be a positive value. b) How much energy is released when 20.00 g of NH3(g) is made to react with an excess of steam to form HNO3 and H2 gases? Again, enter this as a positive value. HNO3(g) + 4H2(g) → NH3(g) + 3H2O(g) ΔH = –637 kJ
Which one of these processes corresponds to the lattice energy of NaCl(s)? O NaCI(s) → Na*(g) + CI (g) O Na(s) + ½ Cl2(g) NaCl(s) O Na*(g) + CI(g) → NaCl(s) O NaCl(s) → Na(s) + ½ Cl2(g)
Given the following data: Fe₂O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g) 3 Fe₂O3(s) + CO(g) → 2 Fe3O4(s) + CO₂(g) Fe3O4(s) + CO(g) → 3 FeO(s) + CO₂(g) calculate AH for the reaction FeO(s) + CO(g) kJ Fe(s) + CO₂(g). ΔΗ = -23 kJ AH = -39 kJ ΔΗ = +18 kJ
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