2. Consider the decomposition of hydrogen sulfide: 2H2S(g) = 2H2(g) + S2(g) Kc = 1.67x107 at 800°C A 0.500L reaction vessel initially contains 0.0125 mol of H₂S at 800°C. Find the equilibrium concentrations of H₂ and S2. Ans: [S₂] = 2.97 x 104 M and [H₂] = 5.94 x 104 M 0.0125 mol 0.025M OSOOL

2. Consider the decomposition of hydrogen sulfide: 2H2S(g) = 2H2(g) + S2(g) Kc = 1.67x107 at 800°C A 0.500L reaction vessel initially contains 0.0125 mol of H₂S at 800°C. Find the equilibrium concentrations of H₂ and S2. Ans: [S₂] = 2.97 x 104 M and [H₂] = 5.94 x 104 M 0.0125 mol 0.025M OSOOL

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 28P

See similar textbooks

Similar questions

A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.
The following two diagrams represent the composition of an equilibrium mixture for the reaction A2 + B2 2AB at two different temperatures. Based on the diagrams, is the chemical reaction endothermic or exothermic? Explain your answer using Le Chteliers principle. (A atoms are red and B atoms are green in the diagrams.)
The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures given: atT=25°C,K= 2.8 X 104 at T = 500°C, A = 2.4 X IO"7 At which temperature are reactants favored? At which temperature are products favored? YVhat can you say about the reaction if the equilibrium constant is 1.2 at 127°C?
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
Consider the same reaction as in Question 11. In one experiment 1.0 mole of H2O(g) and 1.0 mole of CO(g) are put into a flask and heated to 350C. In a second experiment 1.0 mole of H2(g) and 1.0 mole of CO2(g) are put into another flask with the same volume as the first. This mixture is also heated to 350C. After equilibrium is reached, will there be any difference in the composition of the mixtures in the two flasks?
Kc for the decomposition of ammonium hydrogen sulfide is 1.8 104 at 25 C. NH4HS(s) NH3(g) + H2S(g) (a) When the pure salt decomposes in a flask, what are the equilibrium concentrations of NH3 and H2S? (b) If NH4HS is placed in a flask already containing 0.020 mol/L of NH3 and then the system is allowed to come to equilibrium, what are the equilibrium concentrations of NH3 and H2S?
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
The equilibrium constant for the butane iso-butane equilibrium at 25 C is 2.50. Calculate rG at this temperature in units of kJ/mol.