Home
Class 12
CHEMISTRY
Calculate the equilibrium constant for t...

Calculate the equilibrium constant for the cell reaction :
`4Br^(-)+O_(2)+4H^(+)rarr2Br_(2)+2H_(2)O."Given "E_(cell)^(@)=0.16 V`

Text Solution

Verified by Experts

log `K_(c) = (nE_("cell")^(@))/(0.0591)`
`E_("cell")^(@) = 0.16V, n=4`
log `K_(c) = (4 xx 0.16)/(0.0591) = 10.8`
`K_(c) = " antilog" 10.8 = 6.31 xx 10^(10)`
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    AAKASH INSTITUTE|Exercise Try Yourself|19 Videos

  • ELECTROCHEMISTRY

    AAKASH INSTITUTE|Exercise Assignment (SECTION A) Objective Type Questions (One option is correct)|43 Videos

  • COORDINATION COMPOUNDS

    AAKASH INSTITUTE|Exercise Assignment (Section-J Aakash Challenger Questions )|10 Videos

  • ENVIRONMENTAL CHEMISTRY

    AAKASH INSTITUTE|Exercise ASSIGNMENT (SECTION-D) (Assertion - Reason Type Questions)|5 Videos

Similar Questions

Explore conceptually related problems

Calculate the equilibrium constant for the reaction: 3Sn(s) +2Cr_(2)O_(7)^(2-) +28 H^(+) rarr 3Sn^(+4) +4Cr^(3+) +14H_(2)O E^(@) for Sn//Sn^(+2) = 0.136 V E^(@) for4 Sn^(2+)//Sn^(4+) =- 0.154V E^(@) for Cr_(2)O_(7)^(2-)//Cr^(3+) = 1.33V

Determine the value of equilibrium constant for the reaction 2Br^(-)(aq)+I_(2)(s)hArr Br_(2)(l)+2I^(-)(aq)E_("cell")^(@)=-0.54v

Calculate the equilibrium constant for the following reaction: 3Sn + 2Cr_(2)O_(7)^(2-) + 28H^(-) rarr 3Sn^(4+) + 4Cr^(3+) + 14H_(2)O E_(Sn//Sn^(4+))^(@)= 0.009 V, " " E_(Cr_(2)O_(7)^(2-)//Cr^(3))^(@) = 1.33V

The equilibrium constant for the reaction CaSO_(4).5H_(2)H_(2)O(s)hArr CaSO_(4).3H_(2)O(s)+2H_(2)O(g) is equal to

Calculate DeltaG^(@) for the given reaction occuring in fuel cell (i) O_(z) + 4H^(+) + 4e^(-) rarr 2H_(2)O E^(@) = 1.229 volt (ii) 2H_(2) rarr 4H^(+) + 4e^(-) " " E^(@) = 0 volt