CHEMISTRY

posted by .

Explain, in terms of particles, concentration, and reaction rate, what you expect to happen when methane gas (CH4) and hydrogen sulfide gas (H2S) are sealed in a flask and reach a state of equilibrium.

CH4 (g) +2 H2S (g) --><--- CS2 (g) + 4 H2 (g)

  • CHEMISTRY -

    reaction rates each way are equal, by definition of equilibrium.

    pressure will be greater at equilibrium, as (balanced equation) there were 3 moles on left, 5 moles on right, so to whatever degree it goes to the right, it makes more particles, and increases pressure.

  • CHEMISTRY -

    fsj```994994jnc

  • CHEMISTRY -

    BASEDGOD

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chem

    Elemental Sulfur can be formed through the combustion of Hydrogen Sulfide (found in Methane gas) give in equation H2S+O--->S + H2 4 tell how much sulfur is made from 250 grams of methane 2 H2S + O2---->2S +2 H2O s=32
  2. chemistry(check my work)

    The initial concentration for the compounds involved in the reaction shown were determined to be [CS2(g)] = 1.075 mol/L, [H2(g)] = 1.436 mol/L, [CH4(g)] = 0.6740 mol/L, [H2S(g)] = 0.3120 mol/L. Calculate the value of the equilibrium …
  3. chemistry

    Heterogenous equilibrium of ammonium bisulfide. Ammonium bisulfide NH4HS forms ammonia NH3 and hydrogen sulfide H2S through the reaction NH4HS(s) arrows + H2S(g). This reaction has a kp value of 0.120 at 25 C. A 5.0-L flask is charged …
  4. Chemistry

    Explain, in terms of particles, concentration, and reaction rate, what you expect to happen when methane gas (CH4) and hydrogen sulfide gas (H2S) are sealed in a flask and reach a state of equilibrium. CH4 (g) +2 H2S (g) CS2 (g) + …
  5. chemistry

    Ammonium bisulfide, NH2HS, forms ammonia NH3, and hydrogen sulfide, H2S through the reaction: NH4HS (s) <--> NH3(g) + H2S(g) Kp value of .120 at 25C in a 5L flask is charged with .300g of H2S at 25C. A) What are the partial pressures …
  6. Chemistry

    Need help in AP chemistry on Equilibrium When heated, hydrogen sulfide gas decomposes according to the equation 2 H2S(g) ⇄ 2 H2(g) + S2(g) A 3.40 g sample of H2S(g) is introduced into an evacuated rigid 1.25 L container. The …
  7. Chemistry

    Explain, in terms of particles, concentration, and reaction rate, what you expect to happen when methane gas (CH4) and hydrogen sulfide gas (H2S) are sealed in a flask and reach a state of equilibrium. CH4 (g) +2 H2S (g)<=> CS2 …
  8. Chem

    Methane and Hydrogen Sulfide react at 960 degree Celsius and come to the following equilibrium CH4(g)+2H2S(g) <-> CS2(g)+ 4H2(g) At Equilibrium the concentration measured as [Ch4]= 5.56M [H2s]= 11.12 [CS2]= 2.44M [H2] 1.76, A) …
  9. Chemistry

    When CH4(g) (0.06318 mol/L) and 16.43 mol of H2S(g) in a 130.0 L reaction vessel at 711.0 °C are allowed to come to equilibrium the mixture contains 0.04107 mol/L of CS2(g). What is the equilibrium concentration (mol/L) of H2S(g)?
  10. AP chemistry

    Hydrogen sulfide decomposes according to the following reaction, for which Kc = 9.30 10-8 at 700°C 2 H2S(g) 2 H2(g) + S2(g) If 0.51 mol H2S is placed in a 3.0 L container, what is the equilibrium concentration of H2(g) at 700°C?

More Similar Questions