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The minimum voltage required to electrol...

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

A

1.575 V

B

1.60 V

C

1.312 V

D

`-2.62 V`

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The correct Answer is:
B
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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]

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.]

(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"

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

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

Generally alkali metals form their oxides by an average increment of 6 kJ mol^(-1) K^(-1) in their entropies. If at 25^(@)C, Delta G_(f)^(@) of Al_(2)O_(3)(s)=-1582 kJ mol^(-1) , Delta H_(f)^(@) of Li_(2)O(s)=1244 kJ and Delta H_(f)^(@) of Na_(2)O(s)=1411 kJ . The aluminium oxide can be reduced to Al metal by

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)]

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

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?

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