Which of the following equilibria would be impacted by a change in pressure? select the correct answer below: h2(g)+i2(g)→2hi(g) no(g)+o3(g)→no2(g)+o2(g) 2so3(g)→2so2(g)+o2(g) co(g)+h2o(g)→co2(g)+h2

Based on Le Chatelier's principle the following factors affect the equilibrium of a chemical reaction:

1) Temperature

2) pressure

3) change in concentration

4) catalyst

In the given examples, the reactants and products are in the gas phase. In a, b and d the number of moles of reactants is equal to the number of moles of the products. However, in (c) number of moles of products is greater than the reactants. Hence, its equilibria will be affected the most by a change in pressure.

Ans (c)

2SO3(g) → 2SO2 (g) + O2(g)

here we have to get the change of moles on decrease the volume of the reaction in gas phase.

the   per the given options it will decrease by (d) 11-50%

we know, on decreasing the volume of the gas phase reaction the reaction moves to the product side.

the reaction:                     so₂cl₂ (g) = so₂ (g) + cl₂ (g)         total

the moles at equilibrium:   1 - α                 α               α           = 1+α

concentrations:                   1 - α               α               α           = 1 + α

(concentration = moles/volume, as volume is 1 l)

(where α is the degree of dissociation)

now the dissociation constant in terms of concentration is :

=  

or,

or,   = (at v = 1l)

the reaction:                     so₂cl₂ (g) = so₂ (g) + cl₂ (g)         total

the moles at equilibrium:   1 - α                 α               α           = 1+α

concentrations:               (1 - α)/0.5           α/0.5         α/0.5       = (1 + α)/0.5

thus, the dissociation constant in terms of concentration is :

or,  

=  

so, the change of 1 : 1/0.5

or, 1: 2

thus it will decrease by 50%.

or, as per the given options it will decrease by 11-50%

43.452

step-by-step explanation:

284 times .153 = 43.452