Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas. pcl3(g) + cl2(g) equilibrium reaction arrow pcl5(g) a gas vessel is charged with a mixture of pcl3(g) and cl2(g), which is allowed to equilibriate at 450 k. at equilibrium the partial pressures of the three gases are ppcl3 = 0.124 atm, pcl2 = 0.157 atm, and ppcl5 = 1.30 atm.

The question is incomplete, here is the complete question:

Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas:

A gas vessel is charged with a mixture of and , which is allowed to equilibriate at 450 K. At equilibrium the partial pressures of the three gases are = 0.126 atm , = 0.156 atm , and = 1.60 atm. What is the value of at this temperature?

The for the given reaction is 81.4

Explanation:

For the given chemical equation:

The expression of for above reaction follows:

We are given:

Putting values in above equation, we get:

Hence, the for the given reaction is 81.4

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation:

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