Calculate the cell potential (in V) if `/_\` G=-96.5kJ/mol and n=1

Calculate the cell potential (in V) if /_\G=-96.5 kJ/mol and n=1

Calculate the cell potential (in V) if DeltaG = - 96.5 kJ/mol and n = 1.

Calculate the standard enthalpy of formation of n- butane. Given : standard enthalpy of combustion of n- butane, C (graphite) and H_(2)(g) " are " -2878.5 " kJ mol"^(-1), -393.5 " kJ mol"^(-1) and -285.8 " kJ mol"^(-1) respectively.

the bond enthalpy of H_(2)(g) is 436 kJ "mol"^(-1) and that of N_(2)(g) is 941.3 kJ"mol"^(-1) . Calculate the average bond enthalpy of ann N-H bond in ammonia, Delta_(t)^(@)(NH_(3)) =-46 kJ "mol"^(-1)

the bond enthalpy of H_(2)(g) is 436 kJ "mol"^(-1) and that of N_(2)(g) is 941.3 kJ"mol"^(-1) . Calculate the average bond enthalpy of ann N-H bond in ammonia, Delta_(t)^(@)(NH_(3)) =-46 kJ "mol"^(-1)

For the reaction N_(2)H_(4) (g) rarr N_(2)H_(2)(g) +H_(2)(g)" "Delta_(r)H^(@)=109 KJ//mol Calculate the bond enthalpy of N=N . Given : B.E. (N-N) =163 KJ//mol, B.E. (N-H) =391 KJ//mol, B.E. (H-H)=436 KJ//mol

Calculate the change in entropy for the following process : 2 mol of N_(2) (l , 1 atm, -195.6^(@)C) to 2 " mol of " N_(2) (g, 1 " atm " -195.6^(@)C) [Given that, change in molar enthalpy for the vaporisation of N_(2)= 5.586 " kJ mol"^(-1) ]

Calculate the value of enthalpy of combustion of cyclopropane at 25^(@)C and 1 atm pressure. Given: Standard enthalpy of formation of CO_(2)(g),H_(2)O(l) & propene (g) at 25^(@)C are -393.5kJ*mol^(_1),-285.8kJ*mol^(-1)& 20.4kJ*mol^(-1) respectively. also standard enthalpy change for isomerisation reaction: Cyclopropane (g) hArr Propene (g) is -33.0kJ*mol^(-1) .