The reduction of stannous sulphide by hydrogen takes place as follows:SnS(s) + H2(g) 2 Sn(1) + H2S(g)The equilibrium constant (K) values was determined after studying the reaction over thetemperature range 533 to 679°C.The following data was recorded:T/°CK (x 104)53310.658216.163127.667946.2Use the data to determine the enthalpy change (kJ mol-1) for the reaction.

The relationship between equilibrium constant and temperature under two different conditions is…

Answered: The reduction of stannous sulphide by…

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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The table below provides data for the enthalpy and entropy of formation of compounds A and B at standard conditions (298 K) Compound DHfo (kJ mol-1) Sfo(J K-1mol-1) A –135.2 189.2 B –157.6 192.1 (b) A reversible isomerization reaction converts reactant A to product X. Calculate the Gibbs energy change at non-standard conditions (310 K) if the concentration of A is 2 x 10-4M and that of X is 3 x 10-6 M. Comment on whether the reaction is spontaneous at these conditions. The equilibrium constant Keq = 0.05. Assume standard temperature is 298K.
For the triose phosphate catalyzed reaction: dihydroxyacetone phosphate <--> glyceraldehyde-3-phosphate the standard change in Gibbs free energy is ΔG'º=7.53 kJ/mol. Calculate the ΔG for this reaction at 298K when the concentration of dihydroxyacetone phosphate is 0.161 M and the concentration of glyceraldehyde-3-phosphate is 0.00163 M.
The standard Gibbs free energy change is 2.60 kJ/mol for the reaction at 25.0oC: H2(g) + I2(g) →← 2HI(g); ∆Gorxn = + 2.60 kJ/mol The reaction starts with equal molar amounts of H2(g) and I2(g) in a previously evacuated, constant volume vessel. What is the equilibrium mole fraction of HI? Enter your answers with correct units and significant figures.
Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 10. What is the ∆S⁰ in the combustion of hydrogen in the presence of excess oxygen yields water: 2H2(g) + O2(g) → 2H2O(l) in J/K?
1. The equilibrium constant of the reaction 2 C3H5 (g) = C2H4 (g) + C4H8 (g) is found to fit the expression ln K = - 1.04 - (1088 / T) + (1.51 x 105 / T^2 ) between 300 K and 600 K. Calculate the standard reaction enthalpy and standard reaction entropy at 400 K. [2.77 kJ mol-1 ; -16.5 kJ K-1 mol-1 ]
Write a balanced chemical reaction in which iron metal reacts with hydrogen sulfide gas to produce pyrite and hydrogen gas. Using the database of Robie and Hemingway (1995), what is the log of the equilibrium 10 ratio of the fugacities of hydrogen gas to hydrogen sulfide gas at 298.15 K? Assume ideal gases, and activities of solids = 1. What is the enthalpy of reaction for this relationship at 298.15K, in kJ ?
The value of the equilibrium constant at 25ºC, corresponding to the reaction: 3 C2H2 (g) = C6H6 (g), is Keq = 1.22 Taking into account this information, indicate V or F as appropriate,Justify:I) The Gibbs free energy of this reaction is = 0II) The Gibbs free energy of this reaction is <0III) The reaction is spontaneous to the rightIV) It is advisable to manufacture benzene under these conditions.a) TFTF b) TTTT c) FFTT d) FTTT e) FTFT f) TFTT g) TFFF
Ethanoic acid (acetic acid) was evaporated in container of volume 21.45 cm3 at 437 K and at an external pressure of 101.9 kPa, and the container was then sealed. The mass of acid present in the sealed container was 0.0519 g. The experiment was repeated with the same container but at 471 K, and it was found that 0.0380 g of the acid was present. Calculate the equilibrium constant for the dimerization of the acid in the vapour, and the standard enthalpy of the dimerization reaction.
Calculate the equilibrium constant reaction CO(g) + H2(g) H2CO(g), given that for the production of liquid methanal, ∆rG −◦ = +28.95 kJ mol−1 at 298 K and that the vapor pressure of methanal is 1500 torr at the given temperature.
The entropy of reaction at T=198.15K and a pressure of 5 bar.
Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Carbon C2H2(g) 226.7 209.2 200.8 CO2(g) -393.5 -394.4 213.6 Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 What is the ∆S⁰ in the combustion of ethene in the presence of excess oxygen yields carbon dioxide and water: C2H2(g) + 3O2(g) → 2CO2(g) + 2H2O(l) in J/K?
For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data: ΔrH∘ΔrH∘ 182.6kJ mol−1 ΔrS∘ΔrS∘ 24.80J K−1 mol−1 T= 7363 K. Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C∘C:? N2(g)+O2(g)→2NO(g) Express your answer numerically to three significant figures.

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