chemistry

posted by .

A mixture of 1.441 g of H2 and 70.24 g of Br2 is heated in a 2.00-L vessel at 700 K. These substances react as follows.
H2(g) + Br2(g) arrow 2 HBr(g)
At equilibrium the vessel is found to contain 0.627 g of H2.
calculate their equilibrium concentrations and Kc

  • chemistry -

    mols H2 @ equil = 0.627g/2 = 0.3135
    M H2 @ equil = 0.3135/2L = 0.1567M
    M H2 begin = (1.441/4) = 0.360M
    M Br2 begin = (70.24/159.8) = 0.440M

    ........H2 + Br2 ==> 2HBr
    I.....0.36..0.44.....0
    C.....-x.....-x.......2x
    E...0.36-x..0.44-x...2x
    At equil (H2) = 0.157M; therefore, we know
    0.36-x = 0.157 and we solve for x. Use that to calculate each of the equilibrium values, substitute those into the Kc expression and calculate Kc.

  • chemistry -

    Be sure and check (confirm) those numbers. I just ran them one time on my calculator.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    The initial pressure of BrCl(g) in a reaction vessel is 1.6 mbar. If the vessel is heated to 500 K, what is the equilibrium composition of the mixture?
  2. chemistry

    At 1285 degree C the equilibrium constant for the reactin Br2(g) <> 2Br(g) is Keq= 1.04 * 10^-3. A 0.200 L vessel containing an equilibrium mixture of the gases has 0.245 Br2(g) in it. What is the mass of Br(g) in the vessel?
  3. Chemistry

    At 1285°C, the equilibrium constant for the reaction Br2 (gas) <---> 2Br (gas) is Keq= 1.04 X 10^ -3 A 0.200-L vessel containing an equilibrium mixture of gases has 0.245 g. Br2 (gas) in it. What is the mass of Br (gas) in the …
  4. chemistry

    A 0.10-mol sample of H2(g) and a 0.10-mol sample of Br2(g) are placed in a 2.0-L container. The reaction H2(g) + Br2(g) <----> 2 HBr(g) is then allowed to come to equilibrium. A 0.20 mol sample of HBr is placed into a second …
  5. chemistry

    the equilibrium constant for the synthesis of HBr(g0 from hydrogen and bromine gas is 2.18*10 exponent 6 at 730 degrees celcius.if 3.75 mol of HBr(g) is put into a 15L reaction vessel,calculate the concentration of H2,Br2 and HBr at …
  6. Chemistry

    A 0.960mol quantity of Br2 is added to a 1.00 L reaction vessel that contains 1.23mol of H2 gas at 1000 K. What are the partial pressures of H2, Br2, and HBr at equilibrium?
  7. AP Chemistry

    For 2 SO2(g) + O2(g) equilibrium reaction arrow 2SO3(g), Kp = 3.0 104 at 700. K. In a 2.00-L vessel the equilibrium mixture contains 1.11 g of SO3 and 0.106 g of O2. How many grams of SO2 are in the vessel
  8. AP Chemistry

    For 2 SO2(g) + O2(g) equilibrium reaction arrow 2SO3(g), Kp = 3.0 104 at 700. K. In a 2.00-L vessel the equilibrium mixture contains 1.11 g of SO3 and 0.106 g of O2. How many grams of SO2 are in the vessel
  9. chemistry

    equilibrium constant = 2.180 x 10^6 @ 730 C. H2 (g) + Br (g) <=> 2HBr (g) (reversible) startin with 3.20 moles of HBr in a 21.3-L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium idk how to start …
  10. AP Chem

    A mixture of 1.380 g of H2 and 66.80 g of Br2 is heated in a 2.00-L vessel at 700 K. These substances react as follows. H2(g) + Br2(g) equilibrium reaction arrow 2 HBr(g) At equilibrium the vessel is found to contain 0.605 g of H2. …

More Similar Questions