For the equilibrium reaction PCl5(g) (equilibrium arrow)-> PCl3(g) + Cl2(g) explain the effect of increasing the concentration of Chlorine gas using the equilibrium constant.

Kc=[Cl2(g)][PCl3(g)]/[PCl5(g)] for this reaction. The rate constant is not affected by changes in concentration and hence an increase in the concentration of Chlorine causes an increase in the concentration of PCl5(g) to restore equilibrium. This is in accordance with Le Chatelier's principle (change in the system causes shift in equilibrium to oppose it) as the equlibrium has shifted towards the reactant side of the equation. 

JH
Answered by James H. Chemistry tutor

12711 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

24.5g of CH3CH2CH2Br was reacted with ammonia to form CH3CH2CH2NH2 at a 75.0% yield, calculate the mass of the product formed.


What is the basis of an NMR spectrum?


Describe a two step reaction route that can convert 1-Butene (CH2CHCH2CH3) into a compound that is more soluble in water. Use mechanisms to aid your answer (HINT: one of the steps involves nucleophilic substitution)


what is the shape and bond angle of NH3 and use VSEPR theory to explain the bond angle.


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences