Phosphorus pentachloride decomposes according to the chemical equation pcl5(g)↽−−⇀pcl3(g)+cl2(=1.80 at 250 ∘c a 0.197 mol sample of pcl5(g) is injected into an empty 2.90 l reaction vessel held at 250 ∘c. calculate the concentrations of pcl5(g) and pcl3(g) at equilibrium.

The concentration of  is 0.0655 M and  is 0.00240 M at equilibrium.

Given:

Moles of phosphorus pentachloride added to flask = 0.197 mol

The volume of the flask = 2.90

To find:

The concentrations of and at equilibrium.

Solution:

Initial concentration of phosphorus pentachloride in flask:

The equilibrium constant of the reaction =

The equilibrium concentration of phosphorus trichloride =

The equilibrium concentration of chlorine gas =

The equilibrium concentration of phosphorus pentachloride

The expression of an equilibrium constant will be given as:

The equilibrium concentration of phosphorus pentachloride:

The equilibrium concentration of chlorine gas :

The concentration of  is 0.00240 M and  is 0.0655 M at equilibrium.

Learn more about the equilibrium constant here:

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[Cl₂] = 0.0656 mol·L⁻¹; [PCl₅] = 0.002 37 mol·L⁻¹

Explanation:

The balanced equation is

PCl₅ ⇌ PCl₃ + Cl₂

Data:

Kc = 1.80

n = 0.197 mol

V = 2.90 L

1. Calculate the initial concentration of PCl₅

Step 2. Set up an ICE table.

Step 3. Calculate the equilibrium concentrations

[Cl₂] = x mol·L⁻¹ = 0.0656 mol·L⁻¹

[PCl₅] = (0.06793 - 0.0656) mol·L⁻¹ = 0.00237 mol·L⁻¹

Check:

Close enough.

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answer: e.   sour taste

explanation: acids are those substances which dissociates in water to give ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. acids are sour in taste. example: hcl

bases are those substances which dissociates in water to give ions or accepts ions. as they dissociate to give ions, they act as electrolytes and thus are electrically conductive. bases are bitter in taste. bases are slippery in nature.