the concentration equilibrium constant, Kc, is 0.01234 at 727°C for the following system,
CH4 (g) + 2 H2S (g) <-----> CS2 (l) + 4 H2 (g)
what is the pressure equilibrium constant, Kp, at the same temperature?
the concentration equilibrium constant, Kc, is 0.01234 at 727°C for the following system, CH4 (g) +...
Equilibrium and ICE Table 1) The equilibrium constant (KC) at 1280 °C for the following reaction is 1.1 x 10-3. What are the equilibrium concentrations for Br2(g) and Br(g) if the initial concentration of Br2 is 0.125 M? Br2(g) ⇌ 2 Br(g) 2) Consider the reaction for the decomposition of H2S at 800 °C where the KC is 1.67 x 10-7. In a 0.5 L reaction vessel the initial concentration of H2S is 0.0125 mol at 800 °C. What are...
Consider the following reaction: CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g)A reaction mixture initially contains 0.50 M CH4 and 0.75 M H2S. If the equilibrium concentration of CS2 is 0.15 M, what is the equilibrium constant (Kc) for the reaction.Hint: You might need an I.C.E. Table for this one. please show work
Consider the following reaction: CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g) A reaction mixture initially contains 0.800 M CH4 and 0.950 M H2S. If the equilibrium concentration of H2 is 0.440 M, find the equilibrium constant (Kc) for the reaction. A. A) 0.234 B. B) 0.0381 C. C) 2.93 D. D) 10.2 E. E) 0.0112 F. F) none of these
The equilibrium constant KC for the equation CS2 + 4H2 = CH4 + 2H2S at 900 °C is 27.8. What is the value of KC for the following equation? 1/5CH4 + 2/5 H2S = 1/5CS2 + 4/5H2
QUESTION 1 CH4(g) + 2 H2S(g) = CS2(g) + 4 H2(g) A reaction mixture initially contains 0.55 M CH4 and 0.53 M H2S. If the equilibrium concentration of H2 is 0.48 M, find the equilibrium constant (Kc) for the reaction. *Please report 3 significant figures. Numbers only, No unit. No scientific notation.
A mixture of 0.01341 mol of CH4, 0.01170 mol of H2S, 0.02118 mol of CS2, and 0.02835 mol of H2 is placed in a 1.0-L steel pressure vessel at 3416 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g) 1 CS2(g) + 4 H2(g) At equilibrium 0.003198 mol of H2S is found in the reaction mixture. - Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2. - Calculate KP for this reaction.
1) 2) 3) 4) The equilibrium constant for the gas phase reaction 2803 (g) = 2802 (g) + O2 (g) is Keg = 7.1 x 102 at 999 K. At equilibrium,_ O only reactants are present O roughly equal amounts of products and reactants are present products predominate only products are present reactants predominate QUESTION 20 The rate law of a reaction is rate = k[X]-. The units of the rate constant are O mol L-15-2 OL mol-15-1 O mol2...
10. 0/4 Submissions Used -/0.09 points A mixture of 0.01270 mol of CH4, 0.01129 mol of H2S, 0.02016 mol of CS2, and 0.02436 mol of H2 is placed in a 1.0-L steel pressure vessel at 3625 K. The following equilibrium is established: 1 CH4(g)2 H2S(g)1CS2 (g ) +4 H2(g) At equilibrium 0.002399 mol of H25 is found in the reaction mixture (a) Calculate the equilibrium partial pressures of CH4, H25, CS2, and H2 Peq(CH4) Peq(H2S) Peq(CS2) Peq(H2) (b) Calculate Kp...
Consider the following reaction: CH4(g) + H2S(g) ⇌ CS2(g) + H2(g) A reaction mixture initially contains 0.50 M CH4CH4 and 0.75 M H2SH2S. If the equilibrium concentration of H2H2 is 0.44 M, find the equilibrium constant (Kc) for the reaction.
2 H2S(g) + CH4(g) 근 CS2(g) + 4 H2(g) Ke = 3.4 × 10-4 A 0.10 mol sample of each of the four species in the reaction represented above is injected into a rigid, previously evacuated 1.0 L container. Which of the following species will have the highest concentration when the system reaches equilibrium? A) H2S(g) B) CH4(8) C) CS2(8) D) H2(8)