Home
Class 11
CHEMISTRY
Calculate the degree of dissociation and...

Calculate the degree of dissociation and `K_(P)` for the following reaction.
`PCl_(5)(g)iffPCl_(3)(g)+ Cl_(2)(g)``{:(t=0,a,0,0),(t=t,a-x,x,x):}`
Since for a mole, `x` moles are dissociated

Text Solution

AI Generated Solution

To solve the problem, we need to calculate the degree of dissociation (α) and the equilibrium constant \( K_P \) for the reaction: \[ \text{PCl}_5(g) \rightleftharpoons \text{PCl}_3(g) + \text{Cl}_2(g) \] ### Step 1: Define Variables Let: - \( a \) = initial moles of \( \text{PCl}_5 \) - \( x \) = moles of \( \text{PCl}_5 \) that dissociate at equilibrium ...
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    RESONANCE ENGLISH|Exercise (MSPs)|8 Videos

  • CHEMICAL EQUILIBRIUM

    RESONANCE ENGLISH|Exercise Board Level Exercise|33 Videos

  • CHEMICAL EQUILIBRIUM

    RESONANCE ENGLISH|Exercise ORGANIC CHEMISTRY(Alkyl Halide, Alcohol,Phenol,Ether)|27 Videos

  • CHEMICAL BONDING

    RESONANCE ENGLISH|Exercise ORGANIC CHEMISTRY(Fundamental Concept )|6 Videos

  • D & F-BLOCK ELEMENTS & THEIR IMPORTANT COMPOUNDS

    RESONANCE ENGLISH|Exercise Match the column|1 Videos

Similar Questions

Explore conceptually related problems

For the reaction PCl_(5)(g) rightarrow PCl_(3)(g) + Cl_(2)(g)

For the reaction : PCl_(5) (g) rarrPCl_(3) (g) +Cl_(2)(g) :

For the reaction : PCl_(5) (g) rarrPCl_(3) (g) +Cl_(2)(g) :

Unit of equilibrium constant K_p for the reaction PCl_5(g) hArr PCl_3(g)+ Cl_2(g) is

PCl_(5) is 10% dissociated at 1 atm. What is % dissociation at 4 atm . PCl_(5)(g)hArr PCl_(3)(g)+Cl_(2)(g)

The degree of dissociation of SO_(3) is alpha at equilibrium pressure P_(0) . K_(P) for 2SO_(3)(g)hArr2SO_(2)(g)+O_(2)(g) is

1 mole of PCl_(5) taken at 5 atm, dissociates into PCl_(3) and Cl_(2) to the extent of 50% PCl_(5)(g)hArr PCl_(3)(g)+Cl_(2)(g) Thus K_(p) is :

Phosphorus pentachloride dissociates as follows in a closed reaction vessel PCl_5 (g) hArr PCl_3 (g) + Cl_2( g) If total pressure at equilibrium of the reaction mixture is P and degree of dissociation of PCl_5 is x, the partial pressure of PCl_3 will be.

1 mol of Cl_(2) and 3 mol of PCl_(5) are placed in a 100 L vessel heated to 227^(@)C . The equilibrium pressure is 2.05 atm. Assuming ideal behaviour, calculate the degree of dissociation for PCl_(5) and K_(p) for the reaction. PCl_(5)(g) hArr PCl_(3)(g)+Cl_(2)(g)

Phosphorus pentachloride dissociates as follows, ina closed reaction vessel, PC1_(5(g))hArrPC1_(3(g)) + C1_(2(g)) If total pressure at equilibrium of the reaction mixture is P and degree of dissociation of PC1_(5) is x, the partial pressure of PC1_(3) will be: