Reference no: EM13222016
Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation:
PCl5(g) ? PCl3(g) + Cl2(g)
At 250° 0.375 M PCl5 is added to the flask. If Kc = 1.80, what are the equilibrium concentrations of each gas?
[PCl5] = 4.61 M, [PCl3] = 4.23 M, and [Cl2] = 4.23 M
[PCl5] = 0.188 M, [PCl3] = 0.581 M, and [Cl2] = 0.581 M
[PCl5] = 0.0564 M, [PCl3] = 0.319 M, and [Cl2] = 0.319 M
[PCl5] = 1.80 M, [PCl3] = 1.80 M, and [Cl2] = 1.80 M
The Kp for the reaction below is 1.49 × 108 at 100.0°C:
CO(g)+Cl2(g)->COCl2(g)
In an equilibrium mixture of the three gases, Pco = Pcl2 = 2.22 × 10-4 atm. The partial pressure of the product, phosgene (COCl2), is __________ atm.
6.67 × 1011
3.02 × 1015
3.31 × 104
3.31 × 10-16
7.34
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: Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g) ? PCl3(g) + Cl2(g) At 250° 0.375 M PCl5 is added to the flask. If Kc = 1.80, what are the equilibrium concentrations of each gas?
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