college chemistry

posted by .

At 625 K the value of Kc for the equilibrium represented by the balanced equation is 2.50 x 100. Calculate the value of Kp at the same temperature. Express answer in scientific notation.

2NH3(g) = N2(g)+3H2(g)

  • college chemistry -

    Kp = KcRT(delta n) where delta n = n(gas products) - n(gas reactants)

  • college chemistry -

    whats is the boiling point of a solution composed of 17.6g of urea in (NH2)2CO in .300 kg of water

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chem

    I am having problems with these two questions. 1.The value of the equilibrium constant (Kp) as represented by the first chemical equation is 1.58 x 102 at 727 °C. Calculate the value of the equilibrium constant (Kp) for the second …
  2. Chemistry

    The value of the equilibrium constant (Kp) as represented by the first chemical equation is 1.02 x 102 at 727 °C. Calculate the value of the equilibrium constant (Kp) for the second equation at the same temperature. Express answer …
  3. chemistry

    How do you figure out the answer for the reverse reaction?
  4. chemistry

    The value of the equilibrium constant (Kc) as represented by the first chemical equation is 2.70 x 10-3 at 1200 K. Calculate the value of the equilibrium constant (Kc) for the second equation at the same temperature. Express answer …
  5. college chemistry

    The value of the equilibrium constant (Kp) as represented by the first chemical equation is 4.57 x 10-2 at 395 °C. Calculate the value of the equilibrium constant (Kp) for the second equation at the same temperature. Express answer …
  6. college chemistry

    The value of the equilibrium constant, Kc, at a certain temperature is 4.00 x 10-1. Would the reaction as represented by the chemical equation favor reactants or products?
  7. college chemistry

    What volume (in Liters) of hydrogen must react to form 17.0L of ammonia according to the following balanced equation: N2(g) + 3H2(g) --> 2NH3(g) Assume an excess of N2 and that all are at the same temperature and pressure.
  8. Idontgetit

    The value of the equilibrium constant (Kp) as represented by the first chemical equation is 2.00 x 10-2 at 730 K. Calculate the value of the equilibrium constant (Kp) for the second equation at the same temperature. Express answer …
  9. Idontgetit

    At 565 K the value of Kp for the equilibrium represented by the balanced equation is 2.00 x 10-1. Calculate the value of Kc at the same temperature. Express answer in scientific notation. PCl3(g)+Cl2(g) = PCl5(g) ____ x 10 _____
  10. Idontgetit

    At 1650 °C the value of Kc for the equilibrium represented by the balanced equation is 2.38 x 10-1. Calculate the value of Kp at the same temperature. Express answer in scientific notation. CO(g)+H2O(g) = CO2(g)+H2(g) ___ x 10 ____

More Similar Questions