The equilbirium constant for the isomerization reaction = trans 2-butene at selected temperatures are tabulated below. 883 T/K 826 779 733 702 686 K 1.10 1.20 1.36 1.49 1.63 1.72 Calculate the value of AH° and ASº at this temperature range. [-11.5 kJ mol·'; =-12.3 J K-' mol-l]
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![The equilbirium constant for the isomerization reaction
= trans 2-butene
1-butene
at selected temperatures are tabulated below.
883
T/K
826
779
733
702
686
K
1.10
1.20
1.36
1.49
1.63
1.72
Calculate the value of AH° and ASº at this temperature range.
[-11.5 kJ mol-l; =-12.3 J K' mol-']](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0b32edc3-f7ca-4b90-8752-528188d21926%2F7df2ed6e-cf81-498f-9760-11aeaec1cf64%2Fifwftdf_processed.png&w=3840&q=75)
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- The relevant thermodynamic data, under standard conditions, for the reaction H2(g) + ½O2(g) → H2O(g) are summarised below: Entity: H2O(g) ∆hf ° kJ mol−1: −241.81 ∆gf ° kJ mol−1: −228.59 (a) Compute the equilibrium constant K of this reaction at T = 298 K. (b) Compute the corresponding K at 500 K. To simplify your calculations for this temperature, it is suggested you make the appropriate simplifying assumption. State the assumption you have made.10. What is ∆G for the decomposition of CaCO3 at 298K and a partial pressure of CO2 of 4*10-4 bar? ∆Gf0 for CaCO3(s), CaO(s) and CO2(g) are -1129 kJ/mol, -604 kJ/mol and -394 kJ/mol, respectively. CaCO3(s) → CaO(s) + CO2(g) A. 0 B. -131 kJ/mol C. 112 kJ/mol D. 131 kJ/mol E. 150 kJ/mol (Correct answer is C, I'm just looking for an explanation!).Heterogeneous chemical reactionConsider the following reaction to form an industrially important solid product B:A (g) ↔ B (s) + C (g) + D (g)a) How many phases are present?b) What is the maximum amount of solid product B you can make for each mole of A fed to the reactorif the reactor is operating at 400 ºC and 1 bar. Data: K = 10.43 at 400 ºC
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