Home
Class 12
CHEMISTRY
The minimum voltage required to electrol...

The minimum voltage required to electrolyse alumina in the Hall-Heroul process is [Given, `DeltaG^(@)_(f)(A1_(2)O_(3)) =- 1520kJ//mol` and `DeltaG^(@)_(f)(CO_(2)) = 394kJ//mol]`

A

`0.8 V`

B

`1,60 V`

C

`2.8 V`

D

`3.0 V`

Text Solution

Verified by Experts

`(b) 2AI_(2)O_(3)+3C to 4AI + 3CO_(2)`
`Delta_(f)G^(@)=3DeltaG^(@)(CO_(2))`
`=3xx(-394)-2xx(-1520)=1859kJ`
`=1858xx10^(3)J`
`:. nFE^(@) = 1858 xx 10^(3)" "(n=12 "electrons")`
`:. E^(@)=(1858xx10^(3))/(12xx96500)=1.60 V`
Promotional Banner

Topper's Solved these Questions

  • METALLURGY

    BITSAT GUIDE|Exercise Bitsat Archives|6 Videos

  • HYDROCARBONS

    BITSAT GUIDE|Exercise BITSAT Archives|19 Videos

  • NITROGEN CONTAINING COMPOUNDS

    BITSAT GUIDE|Exercise BITSAT Archives|7 Videos

Similar Questions

Explore conceptually related problems

For the reaction: N_(2)O_(4)(g) hArr 2NO_(2)(g) (i)" " In a mixture of 5 mol NO_(2) and 5 mol N_(2)O_(4) and pressure of 20 bar. Calculate the value of DeltaG for the reaction. Given DeltaG_(f)^(@) (NO_(2)) = 50 KJ/mol, DeltaG_(f)^(@) ((N_(2)O_(4)) =100 KJ/mol and T=298 K. (ii) Predict the direction in which the reaction will shift, in order to attain equilibrium [Given at T=298 K, 2.303 "RT" = 5.7 KJ/mol.]

Based on given information DeltaG^(@)_(f)(CaO) =- 604.2kJ//mol and DeltaG^(@)_(f)(A1_(2)O_(3)) =- 1582kJ//mol , which of the following is feasible?

Nitroglycerine (MW =227.1) denotes according to the following equation : 2C_(3)H_(5)(NO_(3))_(3)I to 3N_(2)(g)+1//2O_(2)(g)+6CO_(2)(g)+5H_(2)O(g) The standard molar enthalpies of formation, DeltaH_(f)^(@) for the compounds are given bellow: DeltaH_(f)^(@)[C_(3)H_(5)(NO_(3))_(3)]= -364 kJ//mol DeltaH_(f)^(@)[CO_(2)(g)]= -395.5 kJ//mol DeltaH_(f)^(@)[H_(2)O(g)]= -241.8 kJ//mol DeltaH_(f)^(@)[N_(2)(g)]= 0 kJ//mol DeltaH_(f)^(@)[O_(2)(g)]= 0 kJ//mol The enthalpy change when 10g of nitroglycerine is detonated is

Calculate the heat produced (in kJ) when 224 gm of CaO is completely converted to CaCO_(3) by reaction with CO_(2) at 27^(@) in a container of fixed volume. Given : DeltaH_(f)^(@)(CaCO_(3),s)=-1207kJ//mol," "DeltaH_(f)^(@)(CaO,s)=-635kJ//mol DeltaH_(f)^(@)(CO_(2),g)=-394kJ//mol,["Use R"=8.3JK^(-1)mol^(-1)]

(A) Reduction of Cr_(2)O)(3) with the Aluminium is possible ( R ) DeltaG_((f))^(0) of Cr_(3)O_(3) " is -540kj//mole and" DeltaG_((f))^(0) of Al_(2)O_(3) is -827kj//"mole"

Find DeltaG (J//"mol") for the reaction at 300 kPa and 27^(@)C when all gases are in stoichimetric ratio of moles. N_(2)O_(4)(g)rarr2NO_(2)(g) [ln 2=0.7] Given : DeltaG_(f)^(@)(N_(2)O_(4))=100"kJ/mol" DeltaG_(f)^(@)(NO_(2))=50"kJ/mol" R=8"J/mol"-K

Calculate the pH at which the following reaction will be at equilibrium in basic medium : A_(2)(s) hArr A^(-)(aq) +AO_(3)^(-) (aq) When the equilibrium concentration at 300 K are: [A^(-)] = 0.1M, [AO_(3)^(-)] = 0.1M Given: DeltaG_(f)^(@) of OH^(-)(aq) =- 150 kJ//"mole" , DeltaG_(f)^(@) "of" H_(2)O(l) =- 233 kJ//"mole" DeltaG_(f)^(@) "of" A^(-)(aq) =- 50 kJ//"mole" , DeltaG_(f)^(@) "of" AO_(3)^(-) (aq) =- 123.5 kJ//"mole" , R = (25)/(3) J "mole"^(-1) K^(-1), log_(e) 10 = 2.3