# Standard Enthalpy

Use this for part (a)

N2H4(g) +2 H2O2(l) -> N2(g) + 4 H2O(g)

a) Calculate the enthalpy change, Delta{H}^{o}, for the above reaction using the enthalpy of formation values from the following table.

Delta{H}^{o}f (kJ/mol)

N2H4(g) 95.40

H2O2(l) -187.8

H2O(g) -241.8

I know sort of where to begin on this with standard enthalpy, however I am not quite sure where to go and so I would like some help. Thanks! I have been working to use the formula.

The **standard enthalpy of formation **assignments help is defined as the change in **enthalpy** when one mole of a substance in the **standard** state (1 atm of pressure and 298.15 K) is **formed**from its pure elements under the same conditions.

use this equation

Delta H (reaction) = Sum of enthalpies of formation of the products - sum of enthalpies of formation of the reactants.