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

answer is d because it is trust me

answer: cellular respiration takes in food and uses it to create atp, a chemical which the cell uses for energy. usually, this process uses oxygen, and is called aerobic respiration. it has four stages known as glycolysis, link reaction, the krebs cycle, and the electron transport chain.