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For the reaction N(2)+3X(2) to 2NX(3) wh...

For the reaction `N_(2)+3X_(2) to 2NX_(3)` where X=F, Cl (the average bond energies are F-F = 155 kJ `"mol"^(-1)` N-F = 272 kJ `"mlo"^(-1)`, Cl-Cl = 242 kJ `"mol"^(-1)`, N-Cl= 200 kJ `"mol"^(-1) and N -=N = 941 kJ "mol"^(-1)`), the heats of formation of `NF_(3) and NCl_(3)` in kJ `"mol"^(-1)`, respectively, are closest to

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Given that the food energies of :N-=N is 946kJ "mol"^(-1) , H-H is 435 kJ "mol"^(-1),N-N is 159 kJ "mol"^(-1) , and N-H is 389 kJ "mol"^(-1) , the heat of formation of hydrazine in the phase in kJ "mol"^(-1) is :

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Few values of enthalpies are given below: O=-141 KJ mol^(-1) F= -328 KJ mol^(-1) S= -200 KJ mol^(-1) Cl= -349 KJ mol^(-1) What do these values show?

Few values of enthalpies are given below: O=-141 KJ mol^(-1) F=-328 KJ mol^(-1) S=-200 KJ mol^(-1) Cl=-349 KJ mol^(-1) What do these values show?

Based on the values of B.E. given, Delta_(f)H^(@) of N_(2)H_(4) (g) is : Given : N-N = 159 " kJ mol"^(-1)," "H-H=436 " kJ mol"^(-1) N-=N = 941" kJ mol"^(-1), " "N-H=398 " kJ mol"^(-1)

Based on the values of B.E. given, Delta_(f)H^(@) of N_(2)H_(4) (g) is : Given : N-N = 159 " kJ mol"^(-1)," "H-H=436 " kJ mol"^(-1) N-=N = 941" kJ mol"^(-1), " "N-H=398 " kJ mol"^(-1)

Given that bond energies H-H and Cl-Cl are 430 kJ mol^(-1) and 240 kJ mol^(-1) respecively and Delta_(f) H for HCl is - 90 kJ mol^(-1) . Bond enthalpy of HCl is :