Chemistry-w/addition

posted by .

At elevated temperatures, SbCl5 gas decomposes into SbCl3 gas and Cl2 gas as shown by the following equation: SbCl5(g)<=> SbCl3(g) + Cl2(g)

(a) An 59.8 gram sample of SbCl5 (molecular weight 299.0) is placed in an evacuated 15.0 liter container at 182°C.

1. What is the concentration in moles per liter of SbCl5 in the container before any decomposition occurs?

2. What is the pressure in atmospheres of SbCl5 in the container before any decomposition occurs?

b)If the SbCl5 is 29.2 percent decomposed when equilibrium is
established at 182°C, calculate the values for equilibrium constants Kp and Kc, for this decomposition reaction.
Kc=?
Kp=?

c.In order to produce some SbCl5, a 1.00 mole sample of SbCl3 is first
placed in an empty 2.00 liter container maintained at a temperature
different from 182ºC. At this temperature, Kc, equals 0.117. How many moles of Cl2 must be added to this container to reduce the number of
moles of SbCl3 to 0.500 mole at equilibrium?

  • Chemistry-w/addition -

    1. What is the concentration in moles per liter of SbCl5 in the container before any decomposition occurs?
    moles = grams/molar mass.
    Solve for moles.

    M = moles/L. Solve for M.


    2. What is the pressure in atmospheres of SbCl5 in the container before any decomposition occurs?

    Use PV = nRT. Don't forget to change T to Kelvin.

    b)If the SbCl5 is 29.2 percent decomposed when equilibrium is
    established at 182°C, calculate the values for equilibrium constants Kp and Kc, for this decomposition reaction.
    Kc=?
    Kp=?

    M x fraction decomposed = (SbCl3)
    M x fraction decomposed = (Cl2)
    M x (1.00 - fraction decomposed) = (SbCl5) after decomposition.
    Substitute into the Kc expression below:
    Kc = (SbCl3)(Cl2)/(SbCl5) = Kc

    For Kp, the following:
    You know (Cl2), (SbCl3), and (SbCl5) in M.
    Multiply each by 15.0 L (M x L = moles) to obtain moles of each, then use PV = nRT to obtain the pressure of each. Substitute into the Kp expression.
    Kp = pSbCl2*pCl2/pSbCl5 = ??


    c.In order to produce some SbCl5, a 1.00 mole sample of SbCl3 is first
    placed in an empty 2.00 liter container maintained at a temperature
    different from 182ºC. At this temperature, Kc, equals 0.117. How many moles of Cl2 must be added to this container to reduce the number of
    moles of SbCl3 to 0.500 mole at equilibrium? 1mole/2L = 0.5 M
    .....SbCl5(g) ==>SbCl3(g) + Cl2(g)
    .....0...........0.5M.......0
    .................-x........ +x
    ................0.25M.......y
    What is y? 0.5-x = 0.25
    Solve for x to obtain y.

    Post your work on these if you get stuck.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    Calculate the value of the equilibrium constant (Kc) for the reaction shown, if SbCl5 was found to be 5.57% decomposed at 521K when its initial concentration was 7.60M. SbCl5 <==> SbCl3 + Cl2
  2. Chemistry

    Question: Antimony (V) chloride, SbCl5, dissociates on heating to SbCl5(g)goes to SbCl3(g)+ Cl2(g). A closed 3.50 L vessel initially contains 0.0125 mol SbCl5. what is the total pressure at 248 degree's C when equilibrium is achieved?
  3. chemistry

    1.30 mol each of CO} and Cl2 are introduced into an evacuated 1.80 L flask, and the following equilibrium is established at 668 K. CO + Cl2 +++> COCl2 kp = 22.5 Calculate partial pressure of COCl2. i get about 30.9. but its wrong. …
  4. Chemistry

    At elevated temperatures, SbCl5 gas decomposes into SbCl3 gas and Cl2 gas as shown by the following equation: SbCl5(g)<=> SbCl3(g) + Cl2(g) 1. What is the concentration in moles per liter of SbCl5 in the container before any …
  5. CHEMISTRY

    When SbCl3(g) (4.867 mol) and 0.01217 mol/L of Cl2(g) in a 400.0 L reaction vessel at 958.0 K are allowed to come to equilibrium the mixture contains 0.008586 mol/L of SbCl5(g). What concentration (mol/L) of SbCl3(g) reacted?
  6. chemistry

    A sample of metallic element X, weighing 4.315 g, combines with 0.4810 L of Cl2 gas (at normal pressure and 20.0¢ªC) to form the metal chloride with the formula XCl. If the density of Cl2 gas under these conditions is 2.948 g/L, …
  7. chemistry

    A sample of metallic element X, weighing 4.315 g, combines with 0.4810 L of Cl2 gas (at normal pressure and 20.0¢ªC) to form the metal chloride with the formula XCl. If the density of Cl2 gas under these conditions is 2.948 g/L, …
  8. Chemistry - Equilibrium Constant

    Determine the value of the equilibrium constant (Kp) at 800. K and 1 atm pressure. SbCl3(g) + Cl2(g) -> SbCl5(g) Delta G(o)f (SbCl5) = -334.34 kJ/mol Delta G(o)f (SbCl3) = -301.25 kJ/mol Delta H(o)f (SbCl5) = -394.34 kJ/mol Delta …
  9. Chemistry

    NOCL(g) decomposes to from nitrogen monoxide gas and chlorine gas. The equation is 2NOCL ----> 2NO +Cl2 At a certain temperature the equilibrium constant is 1.60 x 10^-6. Calculate the equilibrium concentrations of all gases if …
  10. chem

    . Antimony pentachloride decomposes according to the following equation. SbCl5 (g) → SbCl3 (g) + Cl2 (g) Suppose that 10.0 g of antimony pentachloride is placed in a 5.00 L container and allowed to establish equilibrium. Calculate …

More Similar Questions