Question #167032

calculate Δ*H *for the formation of one mole of dinitrogen pentoxide from its elements in their stable state at 25°C and 1 atm.

Expert's answer

"N_2+" "5\\over 2" "O_2\\to N_2O_5"

From the equation;

"H_2O\\to H_2+" "1\\over 2" "O"

"2HNO_3\\to N_2O+H_2O"

"N_2+3O_2\\to 2HNO_3"

Cancelling the equations;

"H_2O" "\\to" Equation 1 and 3 cancel

"2HNO_3\\to" Equation 2 and 3 cancel

"1\\over 2" "O_2\\to" Equation 1 and 3 cancel

Cancelling the equations reduces the enthalpy of "O_2" from "6\\over 2" to "5\\over 2"

Adding the enthalpies;

"(+285.8)+(+73.7)+(-348.2)=+11.3kJ"

"\\therefore" "\\Delta H_f=11.3kJ"

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