The E^(@) at 25^(@) for the following reaction at the indicated concentration is 1.50 V. Calculate the DeltaG in kJ at 25^(@) C: Cr(s)+3Ag^(+)(aq,0.1M) rarrAg(s)+Cr^(3+)(aq,0.1M)
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^(+)
The E^(@) at 25^(@) C for the following reaction is 0.22 V. Calculate the equilibrium constant at 25^(@) C : H_(2)(g)+2AgCl(s)to2Ag(s)+2HCl(aq)
A follow parallel path of first-order reactions giving B and C as If the initial concentration of A is 0.25 M , calculate the concentration of C after 5 hr of reaction.
For the cell Zn|ZnCl_(2)(m)|AgCl,E is 1.24V at 25^(@)C and 1.260V at 35^(@)C of m=10^(-3) . Write down the cell reaction and calculate DeltaG, DeltaH, and DeltaS at 25^(@)C .
The temperature coefficient of a reaction is 2 and the rate of reaction at 25° C is 3mol L^(-1) min^(-1) . Calculate the rate at 75^(@) C
The standard free energy change for a reaction is -213.3 KJ mol^(-1) "at" 25^(@)C . If the enthalpy change of the reaction is -217.77 KJ "mole"^(-1) . Calculate the magnitude of entropy change for the reaction in Joule "mole"^(-1)
Calculate E_(cell)^(@) and DeltaG^(@) for the following reaction at 25^(@)C . A^(2+)+B^(+) to A^(3+)+B (Given K_(c)=10^(10) , 1F=96500" C mol"^(-1) )
