Methane (CH4 ) reacts with hydrogen sulfide (H2S) to yield H2 and carbon disulfide (CS2 ),...
Methane (CH4 ) reacts with hydrogen sulfide (H2S) to yield H2 and carbon disulfide (CS2 ), a solvent used manufacturing rayon and cellophane; CH4 (g) + 2 H2S(g) = CS2 (g) + 4 H2 (g). What is the value of Kp at 1000K if the partial pressure in an equilibrium mixture at 1000K are 0.20atm of CH4 , 0.25 atm of H2S, 0.52 atm of CS2 , and 0.10 atm of H2 .
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Methane (CH4 ) reacts with hydrogen sulfide (H2S) to yield H2
and carbon disulfide (CS2 ),...
Determining the Equilibrium Constant K_p: Methane (CH_4) reacts with hydrogen sulfide to yield H_2 and carbon...
Determining the Equilibrium Constant K_p: Methane (CH_4) reacts with hydrogen sulfide to yield H_2 and carbon disulfide, a solvent used in manufacturing rayon and cellophane: CH_4(g) + 2H_2S(g) Equilibrium CS_2(g) + 4 H_2(g) What is the value of K_p at 1000 K if the partial pressures in an equilibrium mixture at 1000 K are 0.20 atm of CH_4, 0.25 atm of H_2S, 0.52 atm of CS_2, and 0.10 atm of H_2?
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 stee...
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.
The initial partial pressures of H2, CS2, H2S, and CH4 in the fixed-volume reaction vessel were...
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.
10. 0/4 Submissions Used -/0.09 points A mixture of 0.01270 mol of CH4, 0.01129 mol of...
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) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g)A reaction mixture initially...
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: CS2 (g) + 4 H2 (g) <====> CH4 (g) + 2 H2S...
Consider the following reaction: CS2 (g) + 4 H2 (g) <====> CH4 (g) + 2 H2S (g) Calculate the value of Keq if the equilibrium concentrations are [CS2] = 0.160, [H2] = 0.350, [CH4] = 0.0100, and [H2S] = 0.0200. a) 0.00357 b) 0.000833 c) 0.0000816 d) 600 e) 0.00167
QUESTION 1 CH4(g) + 2 H2S(g) = CS2(g) + 4 H2(g) A reaction mixture initially contains...
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.
Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction NH4HS(s)⇌NH3(g)+H2S(g) This reaction...
Ammonium bisulfide, NH4HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction NH4HS(s)⇌NH3(g)+H2S(g) This reaction has a Kp value of 0.120 at 25 ∘C. What are the partial pressures of NH3 and H2S at equilibrium, that is, what are the values of PNH3and PH2S, respectively? Enter the partial pressure of ammonia followed by the partial pressure of hydrogen sulfide numerically in atmospheres separated by a comma. What is the mole fraction, χ, of H2S in the gas mixture at...
2 H2S(g) + CH4(g) 근 CS2(g) + 4 H2(g) Ke = 3.4 × 10-4 A 0.10...
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)
Consider the following reaction: CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g) A reaction mixture...
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
Determining the Equilibrium Constant K_p: Methane (CH_4) reacts with hydrogen sulfide to yield H_2 and carbon disulfide, a solvent used in manufacturing rayon and cellophane: CH_4(g) + 2H_2S(g) Equilibrium CS_2(g) + 4 H_2(g) What is the value of K_p at 1000 K if the partial pressures in an equilibrium mixture at 1000 K are 0.20 atm of CH_4, 0.25 atm of H_2S, 0.52 atm of CS_2, and 0.10 atm of H_2?
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.
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...
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.
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)
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