
QUESTION 2 CH4(8) + 2 H2S(g) = CS2(8) + 4H2(8) A reaction mixture initially contains 0.84...
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.
CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g) A reaction mixture initially contains 0.65 M CH4 and 0.82 M H2S. If the equilibrium concentration of H2 is 0.88 M, find the equilibrium constant (Kc) for the reaction. *Please report 3 significant figures. Numbers only, No unit. No scientific notation.
QUESTION 3 CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g) A reaction mixture initially contains 0.65 M CH4 and 0.82 M H2S. If the equilibrium concentration of H2 is 0.88 M, find the equilibrium constant (Kc) for the reaction. *Please report 3 significant figures. Numbers only, No unit. No scientific notation.
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) + 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.
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
For the equilibrium, CH4(g) + 2 H2S(g) = CS2(g) + 4H2(g), the concentrations at equilibrium are (CH4) = 0.3322 M, [H2S] = 0.6644 M, [CS2] = 0.0678 M, and [H2] = 0.2712 Mat 1400.0 K. Calculate K. O 0.167 2.50 x 10-3 C) 4.00 - 103
10.) Consider the following reaction: CH_(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 H, is 0.440 M, find the equilibrium constant (Kc) for the reaction. A) 0.234 B) 0.0381 C) 2.93 D) 10.2 E) 0.0112 F) none of these
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)
The initial partial pressures of H2, CS2, H2S, and CH4 in the fixed-volume reaction vessel were 378, 252, 68, and 54 torr, respectively. The following reaction was allowed to come to equilibrium 4H2(g) + CS2(g) ⇌ 2H2S(g) + CH4(g) Find the value of Kp given that the total pressure of the equilibrium mixture was 646 torr.