CH4(g) + S(g) =CS2 (g) + H2S(g)
balance the equation
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CH4(9) + S(g) → CS2 (g) + H2S(g) A.Balance the equation above. B.Is the sulfur oxidized or reduced in the reaction? C.Given 3.841x1025 molecules of CH4, how many moles is this? Show charges. D.Given 25.15 grams of Sulfur gas, how many moles of H2S could be formed? E.How many liters would the moles of H2S gas(from Part D) occupy at 25.0°C and 1.25 atm? F.What would be the volume(L) of H2S gas (from Part E above) if the temperature was...
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
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
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 .
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
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)
Given the reaction below, answer the following questions. (30 pts) CH4(g) + S(g) ----> CS2 (g) + H2S(g) A.Balance the equation above. B.Is the sulfur oxidized or reduced in the reaction? ___________ Show charges. C.Given 3.841x1025 molecules of CH4, how many moles is this? D.Given 25.15 grams of Sulfur gas, how many moles of H2S could be formed? E.How many liters would the moles of H2S gas(from Part D) occupy at 25.0oC and 1.25 atm? F.What would be the volume(L)...
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.
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
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.