1.5 mole of PCl5 are heated at constant temperature in a closed vessel of 4 litres capacity.At the equilibrium,PCl5 is 35percent dissociated into PCl3 and Cl2.calculate the equilibrium constant.

  1. 👍
  2. 👎
  3. 👁
  1. (PCl5) = 1.5 mols/4 L = 0.375 M.
    0.375 M x 0.35 = 0.131 M
    .......PCl5 ==> PCl3 + Cl2

    Kc = (PCl3)(Cl2)/(PCl5)
    You know x is 0.131 M. Substitute and solve for Kc.
    Post your work if you get stuck.

    1. 👍
    2. 👎
  2. Hey solve completely

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    The equilibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121: PCl5 (g) ↔ PCl3 (g) + Cl2 (g) A vessel is charged with PCl5, giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl3

  2. chemistry

    Calculate no: of moles of cl2 produced at equilibrium when 1 mole of pcl5 is heated in 10 DM vessel kc 0.041

  3. chemistry

    c. A student put 1.18 mole of substance A and and 2.85 mole of substance B into a 10 litre flask which was then closed. The reaction that took place was: A(g)+ 2B(g) 3C(g) + D(g) On analysis the equilibrium mixture at 25 0 C was

  4. physics

    A closed inexpansible vessel contains air saturated with water vapour at 77 degree Celsius.The total pressure in the vessel is 1007mmHg.Calculate the new pressure if the temperature is reduced at 27 degree Celsius (S.V.P of water

  1. Chemistry

    Nitrogen dioxide decomposes on heating according to the following equation 2NO2 (g) ↔ 2NO (g) + O2 (g) When 4 mole of nitrogen dioxide were put into a 1dm3 container and heated to a constant temperature, the equilibrium mixture

  2. Chem II

    PCl5 dissociates according to the reaction: PCl5(g) ↔ PCl3(g) + Cl2(g). One mole of PCl5 was placed in one liter of solution. When equilibrium was established, 0.5 mole of PCl5 remained in the mixture. What is the equilibrium

  3. chemistry

    Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) -----> PCl3 (g)+ Cl2(g) Kc= 1.80 at 250 degrees C A 0.463 mol sample of PCl5(g) is injected into an empty 4.80 L reaction vessel held at 250 °C.

  4. Chemistry

    A 522g piece of copper tubing is heated to 89.5C and placed in an insulated vessel containing 159g of water at 22.8C. Assuming no loss of water and a heat capacity for the vessel of 10.0J/K, what is the final temperature of the

  1. chem sorry the last one did not have the question

    A sample of PCl5 weighing 2.69 grams is placed in a 1.000 liter flask and vaporized completely at 250 o C. The final pressure observed at this temperature is 1.000 atmospheres. Note that some, but not all of the PCl5 decomposes

  2. Chemistry

    For the reaction mole of HI is introduced into a vessel at constant temperature.calculate the no of moles of I2 when equilibrium is reached (Kc=0.0156) Plz help me and give complete solution

  3. Chem/math question - from Sam

    For the following reaction at 600. K, the equilibrium constant, Kp, is 11.5. PCl5(g) = PCl3(g) + Cl2(g) Suppose that 2.510 g of PCl5 is placed in an evacuated 470. mL bulb, which is then heated to 600. K. (a) What would be the

  4. General Chemistry II

    The equillibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121: PCl5(g) --> PCl3(g) + Cl2(g) A vessel is charged with PCl5, giving a initial pressure of 0.123 atm. At equillibrium, the partial pressure of PCl3

You can view more similar questions or ask a new question.