Consider the following reaction: 2SO2(g)+O2(g)⇌2SO3(g) Kp=0.355 at 950 K A 2.75−L reaction vessel at 950K initially contains 0.100 mol of SO2 and 0.100 mol of O2.Calculate the total pressure (in atmospheres) in the reaction vessel when equilibrium is reached.

Answer : The total pressure (in atmospheres) in the reaction vessel when equilibrium reached is, 5.02 atm

Explanation :

First we have to calculate the initial pressure of and

and,

The balanced chemical reaction is:

Initial pressure     2.84        2.84           0

At eqm.              (2.84-2x)  (2.84-x)        2x

The expression of for above reaction follows:

Putting values in expression 1, we get:

x = 0.664

Now we have to calculate the total pressure.

Partial pressure of = (2x) = 2(0.664) = 1.33 atm

Partial pressure of = (2.84-2x) = [2.84-2(0.664)] = 1.51 atm

Partial pressure of = (2.84-x) = [2.84-0.664] = 2.18 atm

Total pressure = Partial pressure of + Partial pressure of + Partial pressure of

Total pressure = 1.33 + 1.51 + 2.18

Total pressure = 5.02 atm

Thus, the total pressure (in atmospheres) in the reaction vessel when equilibrium reached is, 5.02 atm

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the correct answer is a. the ability of electrons to flow throughout the metal.

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it takes on an electronical energy