chemistry

For reactions in solution, molar concentrations are usually used in equilibrium constant
expressions (designated by K or Kc). In gases, partial pressures can also be used (designated
by Kp). Equilibrium partial pressures of NOCl, NO and Cl2 in a container at 300 K are 1.2
atm, 0.050 atm and 0.30 atm, respectively. Calculate a value for the equilibrium constant Kp
for the following reaction.
2 2NO (g) + Cl (g)  2NOCl (g)

asked by alex
  1. I found K =1920
    my question is whether the temperature is being used at all and if it is why?

    posted by alex
  2. My calculator is broken so I can't check your calculation; however, no the temperature is not being used EXCEPT that the value for Kp calculated is at 300 K and no other temperature. Kp and Kc change with T.

    posted by DrBob222

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Nitrogen monoxide reacts with chlorine gas according to the reaction: 2NO (g) + Cl2 (g) ⇔ 2NOCl (g) Kp = 0.27 at 700 K A reaction mixture initially contains equal partial pressures of NO and Cl2 . At equilibrium, the
  2. chemistry

    Introduced into a 1.50L container is 0.100mol PCl5(g). The flask is held at 227degreesC until equilibrium is established. What are the partial pressures and the total pressures of the gases in the flask at the equilibrium.
  3. Chemistry

    A gaseous reaction mixture contains SO2, Cl2, and SO2Cl2 in a 2 L container with the gases having the following partial pressures: P(SO2)=0.35 atm, P(SO2Cl2)=0.19 atm, P(Cl2)=0.24 atm. Kp=91 for the equilibrium system: SO2 (g) +
  4. Chemistry

    What's the difference between the pressure of a system and the partial pressures in relation to Le Chatelier's principles? I know that when the pressure of the system is increased, it goes to the side with less moles/particles and
  5. chemistry

    Introduced into a 1.50L container is 0.100mol PCl5(g). The flask is held at 227degreesC until equilibrium is established. What are the partial pressures and the total pressures of the gases in the flask at the equilibrium.
  6. chemistry

    at an equilibrium mixture of PCl5, PCl3, and Cl2 has partial pressures of 217.0 Torr, 13.2 Torr and 13.2 Torr respectively. a quantity of Cl2 is injected into the mixture, and the total pressure jumps to 263.0 Torr (at the moment
  7. chemistry

    at an equilibrium mixture of PCl5, PCl3, and Cl2 has partial pressures of 217.0 Torr, 13.2 Torr and 13.2 Torr respectively. a quantity of Cl2 is injected into the mixture, and the total pressure jumps to 263.0 Torr (at the moment
  8. CHEMISTRY

    Equilibrium Equation with Partial Pressures PCl3(g) +Cl2(g) <-> PCl5(g)? An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of
  9. HELP!!!!!!!!!

    Introduced into a 1.50L container is 0.100mol PCl5(g). The flask is held at 227degreesC until equilibrium is established. What are the partial pressures and the total pressures of the gases in the flask at the equilibrium.
  10. chem

    Introduced into a 1.50L container is 0.100mol PCl5(g). The flask is held at 227degreesC until equilibrium is established. What are the partial pressures and the total pressures of the gases in the flask at the equilibrium.

More Similar Questions