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Given the following equation and equilibrium constant, 2 H2(g) + S2(o)=2 H2S(g) Kc -1.08 x 107...
Question 18 Given the following equation and equilibrium constant, 2 H2 (9) + S2(9)=2 H2S(g) Kc = 1.08 x 107 Determine Kc for the following reaction. Hy8[g) =H2(g)+{ 5200) 2.70 106 1.35 x 106 3.04 x 10-4 2.31 x 10-8 Question 19 Which of the following will cause this reaction to shift toward products? N2(g) + O2(g) = 2 NO(g) increasing [NO] adding a catalyst decreasing the container volume increasing (N2)
> Click Submit to complete this assessment. Question 22 Given the following equation and equilibrium constant, 2 H2(g) + S2(o)=2 H2S(g) Ke=1.08 x 107 Determine Ke for the following reaction. H25(9) =Hz()+ 526) 2.70 x 106 1.35 X 106 3.04 x 10-4 2.31 x 10-8
8. Consider the reaction: 2 H2S(g) 2 H2(g) +S2(g) Kc = 1.67 x 107 at 800°C What is the value of Kp at this temperature?
For the equilibrium H2(g) + S(s) ⇔ H2S(g), Kc = 6.1 x 105 at 298 K. If the concentrations of H2 and H2S are equal, which of the following statements is true? A. The reaction quotient is 1. B. The concentrations of H2 and H2S can never be equal. C. The concentration of S equals Kc. D. The equilibrium constant equals 1. E. The system is at equilibrium.
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...
2 H2S(g) ⇌ 2 H2(g) + S2(g) Kc = 9.0 × 10−8 at 700°C the initial concentrations of the three gases are 0.500 M H2S, 0.500 M H2, and 0.250 M S2. Determine the equilibrium concentrations of the gases.
Consider the reaction for the decomposition of hydrogen sulfide: 2 H2S(g) ⇌ 2 H2(g) + S2(g) A 0.300 L vessel initially contains 0.450 mol of H2S at 800oC. Find the equilibrium concentration of S2. Kc = 1.67 x 10-7 at 800oC. 1) 3.54 × 10-4 M 2) 0.00204 M 3) 0.00455 M 4) 1.94 × 10-4 M 5) 0.00551 M
Consider the following equilibrium: 2H2(g)+S2(g)?2H2S(g)Kc=1.08
4) The equilibrium constant kc for the reaction H2(g) + Br2(g) = 2HBr(g is 2.18 x 106 at 730°C. Starting with HBr only with (HBr]° = 0.267 M, calculate the concentrations of H2, Brz, and HBr at equilibrium.
1) 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 the equilibrium concentrations of H2, S2, and H2S? 2 H2S(g) ⇌ 2 H2(g) + S2(g) 2) At 350 °C the equilibrium pressure of the following reaction mixture is 0.105 atm. What is the Kp and KC of the for the reaction? CaCO2(s)...