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 at 300 K, N_2O_4(g)hArr2NO_2(g) , the value of DeltaG when concentration of each species is 5 mol/litre, will be (Given: ( DeltaG_(fN_2O_4)^o ) = 120 kJ/mol and ( DeltaG_(fNO_2)^o ) = 70 kJ/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.]

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.]

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?

At 298K, for attainment of equilibrium of the reaction N_(2)O_(4)(g)hArr 2NO_(2)(g) , 5 mol of each of the constituents is taken. Due to this, total pressure of the mixture turns 20 atm. If DeltaG_(f)^(0)(N_(2)O_(4))=100kJ*mol^(-1) and DeltaG_(f)^(0)(NO_(2))=50K(J*mol^(-1)) then- (1) Give the value of DeltaG of the reaction? (2) In which direction will the reaction proceed more to attain equilibrium?

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 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)]