2. Data for the reaction 2 HI (g) → H₂ (g) + I₂ (g) are given in the table below:Reaction temperature (K)298729Chemical speciesH₂ (g)1₂ (g)HI (g)Кс1.26 x 10-32.0 x 10-2AHof (kJ/mol)062.44225.9a. Calculate AH (in kJ/mol) using the AH values given. Show your work, and payattention to sig figs.b. Calculate AH (in kJ/mol) using the yan't Hoff equation. Show your work, and payattention to sig figs.

Answered: Image /qna-images/answer/33bce6f1-7124-4f26-80a2-5ebf3a02ffd7.jpg

2. Data for the reaction 2 HI (g) → H₂ (g) + I₂ (g) are given in the table below: Reaction temperature (K) 298 729 Chemical species H₂ (g) 1₂ (g) HI (g) Кс 1.26 x 10-3 2.0 x 10-2 AHof (kJ/mol) 0 62.442 25.9

2. Data for the reaction 2 HI (g) → H₂ (g) + I₂ (g) are given in the table below: Reaction temperature (K) 298 729 Chemical species H₂ (g) 1₂ (g) HI (g) Кс 1.26 x 10-3 2.0 x 10-2 AHof (kJ/mol) 0 62.442 25.9

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

How much heat (in kJ) will be released (∆H) if 0.4501 mol of NH₃ are mixed with 0.200 mol of O₂ in the following chemical reaction? 4 NH₃ (g) + O₂ (g) → 2 N₂H₄ (g) + 2 H₂O (g) ∆H° = -286 kJ/mol
The reaction written below has a ΔH of +2,662 kJ/mol 6CO2(g) + 6H2O(g) --> C6H12O6(g) +6O2(g) How much energy must be input into this reaction to make 92 grams of C6H12O6(g) ?
10. The enthalpy change for the reaction: H+(aq) + OH-(aq) → H2O (l) ΔH rxn =-57.6 kJ/mol. If 161.4 mL of 0.52 M H3PO4 at 24.17°C is mixed with 169.1 mL of 0.56 M Ba(OH)2 at 24.17°C, what is the maximum temperature reached by the resulting solution if the heat capacity of the calorimeter is 435.6 J/K?
Mothballs are composed primarily of the hydrocarbon naphthalene (C10H8). When 1.167 g of naphthalene burns in a bomb calorimeter, the temperature rises from 25.891 °C to 32.724 °C.
Consider the following reaction: 2 CH3OH(g) → 2 CH4(g) + O2(g) ΔH = +252.8 kJ Is this reaction exothermic or endothermic? Endothermic Calculate the amount of heat transferred when 24.0g of CH3OH is decomposed by this reaction at constant pressure.
How much heat (in kJ) will be released (∆H) if 0.5093 mol of NH₃ are mixed with 0.200 mol of O₂ in the following chemical reaction? 4 NH₃ (g) + O₂ (g) → 2 N₂H₄ (g) + 2 H₂O (g) ∆H° = -286 kJ/mol
Part 2 The Haber process produces ammonia (NH3) for the chemical industry from nitrogen (N₂) and hydrogen (H₂) as shown in the chemical equation below. This is a reversible reaction. N2 (8) + 3H2(g) → 2NH3 (8) AH = -92 kJ mol-¹ (exothermic) The following questions relate to the effect of changing factors that influence the direction of the above reaction, according to Le Chatelier's principle. For each change in factor (i - iv) listed in the Table, you need to: state the direction of equilibrium, give a reason for your choice, identify if the amount of ammonia produced will increase or decrease. Factor Decrease in concentration of N₂ i) ii) Increase in pressure iii) Increase in temperature iv) A catalyst is added Direction (shift) of equilibrium Scientific explanation for stated direction of equilibrium. Amount of NH3 Increases / decreases Part 3 During this reaction, compromises are made to speed up and maximise the production of ammonia. i) ii) Suggest why a moderate amount of…
Determine the standard enthalpy (ΔH) for this reaction and explain the cooling effect that is experienced when methanol is accidentally dropped on the skin. The standard enthalpy of formation for CH3OH(l) is -239.1 kJ/mol and for CH3OH(g) is -189.83 kJ/mol. CH3OH(l) → CH3OH(g)
The reaction written below has a ΔH of +2,971 kJ 6CO2(g) + 6H2O(g) --> C6H12O6(g) +6O2(g) How much energy must be input into this reaction to make 93.087 grams of C6H12O6(g) ? (Input your answer in kJ, but do not include the units in your answer.)
Solid lithium chloride dissolves in water according to the equation below.LiCl (s) ⟶ Li+ (aq) + Cl− (aq) ΔHº = –37.03 kJ/mol5.00 grams of solid LiCl (m.w. = 42.39 g/mol) dissolves in 60.0 grams of water initially at a temperature of 25.00 ºC in a perfect calorimeter. Calculate the final temperature of the solution in the calorimeter.[You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g·ºC)]Tfinal = Answer ºC
Classify the following reactions as endothermic or exothermic.
Please answer question 20 part A