The E^(@) at 25^(@) C for the following reaction is 0.55 V. Calculate the DeltaG^(@) in kJ // mol : 4BiO^(+)(aq)+3N_(2)H_(5)^(+)to4Bi(s)+3N_(2)(g)+4H_(2)O(l)+7H^(+)
Given [CS_(2)]=0.120M,[H_(2)]=0.10,[H_(2)S]=0.20 and [CH_(4)]=7.40xx10^(-5)M for the following reaction at 900^(@) C at eq.Calculate the equilibrium constant (K_(c)) . CS_(2)(g) +4H_(2)(g)->CH_(4)+2H_(2)S(g)
Calculate the standard cell potentials of galvanic cell in which the following reactions take place: Calculate the Delta_rG^ o and equilibrium constant of the reactions. 2Cr(s) + 3Cd^(2+)(aq) rarr 2Cr^(3+)(aq)+ 3Cd
Calculate the standard cell potentials of galvanic cell in which the following reactions take place: Calculate the Delta_rG^o and equilibrium constant of the reactions. Fe^(2+)(aq) + Ag^+ (aq) rarr Fe^(3+) (aq) + Ag(s)
Calculate the equilibrium constant of the reaction: Cu(s) + 2Ag^+(aq) → Cu^(2+) (aq) + 2Ag(s) E^o(cell) = 0.46 V
For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with
Consider the following standard electrode potentials and calculate the eqillibrium constant at 25^(@) C for the indicated disproportional reaction : 3 Mn^(2+)(aq)toMn(s)+2Mn^(3+)(aq) Mn^(3+)(aq)+e^(-)toMn^(2+)(aq), E^(@)=1.51 V Mn^(2+)(aq)+2e^(-)toMn(s), E^(@)=-1.185 V
At a certain temperature , the following reactions have the equilibrium constants as shown below: S(s)+O_(2)(g)hArrSO_(2)(g),K_(c)=5xx10^(52) 2S(s)+3O_(2)(g)hArr2SO_(3)(g),K_(c)=10^(29) what is the equilibrium constant K_(c) for the reaction at the same temperature? 2SO_(2)(g)+O_(2)(g)hArr2SO_(3)(g)
Calculate the equilibrium constant for the reaction 2Fe3+(aq) + 2I– (aq) → 2Fe2+(aq) + I2(s) E0cell = 0.236V
Classify the following reactions as C_2H_4(g) + H_2 rarr C_2H_6 (g)