Calculate the temperature at which DeltaG=-5.2 kJ mol^-1 ,DeltaH=145.6kJ mol^-1 and DeltaS=216 JK^-1 mol^-1 for a chemical reaction
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 enthalpy of formation of ammonia from the following bond enegry data: (N-H) bond = 389 kJ mol^(-1), (H-H) bond = 435 kJ mol^(-1) , and (N-=N)bond = 945.36kJ mol^(-1) .
Calculate the standard enthalpy of combustion of CH_(4) , it standard enthalpies of formation of CH_(4(g)),H_(2)O_((l)), and CO_(2(g)) are -74.81kJ mol^(-1), -285.83kJ mol^(-1) and -393.51kJ mol^(-1) respectively.
Calculate the entropy change for vaporization of 1mol of liquid water to stem at 100^(@)C , if Delta_(V)H = 40.8 kJ mol^(-1) .
The DeltaH_(f)^(0)(KF,s) is -563 kJ mol^(-1) . The ionization enthalpy of K(g) is 419 kJ mol^(-1) . and the enthalpy of sublimation of potassium is 88 kJ mol^(-1) . The electron affinity of F(g) is 322 kJ mol^(-1) and F-F bond enthalpy is 158 kJ mol^(_1) . Calculate the lattice enthalpy of KF(s) . The given data are as follows: (i) K(s)+1//2F_(2)(g)rarrKF(s)" "DeltaH_(f)^(0)= -563 kJ mol^(-1) (ii) K(g)rarrK^(+)(g)+e^(-)" "Delta_("Ioniz")^(0)=419 kJ mol^(-1) (iii) K(s)rarrK(g)" "DeltaH_("sub")^(0)=88kJ mol^(-1) (iv) F(g)+e^(-)rarrF^(-)(g)" "DeltaH_(eg)^(0)= -322 kJ mol^(-1) (v) F_(2)(g)rarr2F(s)" "DeltaH_("diss")^(0)= 158 kJ mol^(-1) (vi) K^(+)(g)+F^(-)(g)rarrKF(s)" " DeltaH_(L)^(0)=?
