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28 Sep 2019
Consider the reaction: PCl5 (g) <--> PCl3 + Cl2 K= 5.0 x 10-2at 240 degrees C.
(A) In an experiment, 0.200 mol of PCl5, 0.500 mol of PCl3, and0.300 mol of Cl2 are mixed in a 2.00 L container. Calculate theequilibrium concentrations of PCl5, PCl3, and Cl2.
Consider the reaction N2O4 (g) <--> 2NO2 (g) at a temperaturewhere Kp = 0.131 atm.
(A) A flask initially contains N2O4 at 1.000 atm pressure.Calculate the pressures of NO2 and N2O4 at equilibrium.
Consider the reaction: PCl5 (g) <--> PCl3 + Cl2 K= 5.0 x 10-2at 240 degrees C.
(A) In an experiment, 0.200 mol of PCl5, 0.500 mol of PCl3, and0.300 mol of Cl2 are mixed in a 2.00 L container. Calculate theequilibrium concentrations of PCl5, PCl3, and Cl2.
Consider the reaction N2O4 (g) <--> 2NO2 (g) at a temperaturewhere Kp = 0.131 atm.
(A) A flask initially contains N2O4 at 1.000 atm pressure.Calculate the pressures of NO2 and N2O4 at equilibrium.
(A) In an experiment, 0.200 mol of PCl5, 0.500 mol of PCl3, and0.300 mol of Cl2 are mixed in a 2.00 L container. Calculate theequilibrium concentrations of PCl5, PCl3, and Cl2.
Consider the reaction N2O4 (g) <--> 2NO2 (g) at a temperaturewhere Kp = 0.131 atm.
(A) A flask initially contains N2O4 at 1.000 atm pressure.Calculate the pressures of NO2 and N2O4 at equilibrium.
Patrina SchowalterLv2
28 Sep 2019