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
The equilibrium constant KC for the equation CS2 + 4H2 = CH4 + 2H2S at 900...
calculate the value for the thermodynamic equilibrium constant for the following reaction. CS2 (g) + 4H2 (g) --> CH4 (g) + 2H2S (g) Values for delta Gf: CS2 (g) --> + 66.85 kJ/mol H2 (g) --> + 0.00 kJ/mol CH4 (g) --> - 50.80 kJ/mol H2S (g) --> - 33.33 kJ/mol R = 8.314 x 10^-3 kJ/molK T = 298 K
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
[References The equilibrium constant K, for the equation CS2 (9) + 4H, (9) CH4(9) + 2H,S(9) at 900°C is 27.8. What is the value of K, for the following equation? CH (9)+ H,() CS, (9)+() K. = Submit Answer Try Another Version 7 item attempts remaining
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 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.
1. At a certain temperature, 0.338 mol CH4 and 0.808 mol H2O is placed in a 4.00 L container. CH4(g)+2H2O(g)????CO2(g)+4H2(g) At equilibrium, 4.89 g CO2 is present. Calculate Kc. 2. At a certain temperature, 0.352 mol CH4 and 0.862 mol H2S are placed in a 1.50 L container. CH4(g)+2H2S(g)????CS2(g)+4H2(g) At equilibrium, 14.5 g CS2 is present. Calculate Kc . 3. At a certain temperature, 0.3211 mol of N2 and 1.501 mol of H2 are placed in a 2.50 L container....
QUESTION 2 CH4(8) + 2 H2S(g) = CS2(8) + 4H2(8) A reaction mixture initially contains 0.84 M CH4 and 0.45 M H2S. If the equilibrium concentration of H2 is 0.64 M, find the equilibrium constant (Ke) for the reaction *Please report 3 significant figures. Numbers only. No unit. No scientific notation
13. Write the equilibrium constant equation for the following reversible reactions.(3 points for the first two equations, 4 for the third equation) a. C2H4 (g) + 3 O2(g) → 2CO2 (g) + 2 H20 (g) b. CS2 (g) + 4H2(g) + 2H2S(g) + CH4(E) c. Ag2CO3 (5) + 2H*(aq) + 2 C1(aq) —2AgCl(s) + CO2(g) + H20(1) HTML Editora
1. Write the equilibrium constant expressions (Kc) for the following reactions: (a) CO (g) + H2O (g) ⮂ CO2 (g) + H2 (g) (b) CH4 (g) + 2H2S (g) ⭢ CS2 (g) + 4H2 (g) (c) COCl2 (g) ⮂ Cl2 (g) + CO (g) (d) 2HI (g) ⮂ H2 (g) + I2 (g) (e) PCl3 + Cl2 (g) ⮂ PCl5 (g) (f) 2H2 (g) + O2 (g) ⮂ ...
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