Hydrogen sulfide is a pollutant found in natural gas. Following its removal, it isconverted to sulfur by the reaction:211,S(g) + SO2(g) S.(s, rhombic) + 2H20(1)What is the equilibrium constant for this reaction? Is the reaction endothermic orexothermic?

Given reaction is : 2H2S (g) + SO2 (g) <------> 38 S8 (s, rhombic) + 2H2O (l) Calculate the…

Hydrogen sulfide is a pollutant found in natural gas. Following its removal. it is converted to sulfur by the reaction: 21,S(g) + SO2(g) S.(s, rhombic) 2H,0(1) What is the equilibrium constant for this reaction? Is the reaction endothermic or exothermic?

Hydrogen sulfide is a pollutant found in natural gas. Following its removal. it is converted to sulfur by the reaction: 21,S(g) + SO2(g) S.(s, rhombic) 2H,0(1) What is the equilibrium constant for this reaction? Is the reaction endothermic or exothermic?

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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7
For the reversible reaction: N 2 (g)+ O 2 (g) = 2 NO (g) AH= 181 kJ (a) What will happen to the concentrations of NO at equilibrium if O, is added? (b) What will happen to the concentrations of NO at equilibrium if NO is removed? (c) What will happen to the concentrations of NO at equilibrium if the volume of the reaction vessel is increased? (d) What will happen to the concentrations of NO at equilibrium if the temperature of the system is decreased? (e) What will happen to the concentrations of N,, 0,, and NO at equilibrium if a catalyst is added?
Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into a 5.00 L flask at 1200 K. The flask is found to contain 2.81 g of CH, 1.25 g of CO, 15.1 g of cO, and 25.3 g of H, What is the value of Kc for this reaction? CH.(g) + CO,(9) = 2 CO(g) + 2 H,(g)
What will happen to the equilibrium, NaHCO3(s)Na2CO3(s) + CO2(g) + H2O(g);Ho = 136 kJ when: (a) the temperature is decreased(b) the volume of the container is increased (c) water vapor is removed(d) additional Na2CO3 is added(e) pressure of CO2 is increased
For which of these reactions will there be no effect on the relative amounts of the substances present at equilibrium when the pressure of the system is increased at constant temperature? O 2 sO, (g) + 0,(g) = 2 SO, (g) + heat heat + CO, (g) + NO(g) =CO(g) + NO, (g) heat + 2 Cl, (g) + 2 H,O(g) = 4 HCI(g) + 0, (g) N, (g) + 3 H, (g) = 2 NH, (g) + heat
Consider the following reversible reaction at equilibrium: C6H12O6(aq) + 6 O2(g) 6 CO2(g) + 6 H2O(l). Given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?
Is this not 5.37?
Consider the following reaction: CO (g) + 2 H₂ (9) CH3OH (g) A reaction mixture in a 5.21 - L flask at a certain temperature initially contains 27.4 g CO and 2.36 g H₂. At equilibrium, the flask contains 8.65 g CH3OH. Calculate the equilibrium constant (K) for the reaction at this temperature. Kc = Submit ΠΑΠ ΑΣΦ 4 Request Answer ?
Please answer ALL parts of the question and show your work. Consider this reaction: 2H2S(g) + 3O2(g) <-----> 2H2O(g) + 2SO2(g) H= -1036 kJ Predict whether the forward or reverse reaction will reestablish equilibrium is disturbed by (a) expanding the container (b) removing SO2 (c) rasing the temperature (d) water vapor is added
Please don't provide handwritten solution ....
Consider the following system: 4 NH3(g) + 3 O2(g) -> 2 N2(g) + 6 H2O(l) AH = -1530.4 kJ (a) How will the amount of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N,(g)? (3) adding water? (4) expanding the container at constant pressure? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
7 4 (a) Calculate the value of Kc for the reaction: PC15 (2) PC13 (g) + Cl2 (g) AH = Positive Given that when 8.4 mol of PCls (g) is mixed with 1.8 mol of PC13 (g) and allowed to come to equilibrium in a 10 dm³ container the amount of PCls (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: (1) Increasing temperature (ii) Lowering the concentration of chlorine (Cl2) (iii) Addition of a catalyst