Phosphine decomposes by the following reaction: COCl2(g) <---> CO(g) + Cl2(g) Kc = 8.3 x 10-4...

Phosphine decomposes by the following reaction:

COCl_2(g) <---> CO_(g) + Cl_2(g) K_c = 8.3 x 10^-4

Calculate the concentration of each component when 2.55 g of phosphine decomposes in a 25.0mL flask.

Solutions

Expert Solution

mass of COCl2 = 2.55 g

moles of COCl2 = 2.55 / 98.92 = 0.0258 mol

concentration = 0.0258 / 0.025 = 1.03 M

COCl2 (g) <-------------> CO (g) + Cl2 (g)

1.03 0 0

1.03 - x x x

Kc = x^2 / 1.03 - x

8.3 x 10^-4 = x^2 / 1.03 - x

x = 0.0292

concentration of compounds :

[COCl2] = 1.00 M

[CO] = 0.0292 M

[Cl2] = 0.0292 M

queen_honey_blossom answered 8 months ago

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