The enthalpy of the decomposition reaction of N2H4 gas is the amount of heat energy released or absorbed during the reaction. It is typically represented by the symbol ΔH and is measured in units of kilojoules per mole (kJ/mol).
The chemical equation for the decomposition reaction of N2H4 gas is 2N2H4(g) → N2(g) + 2H2(g). This means that for every two molecules of N2H4 gas that decompose, one molecule of N2 gas and two molecules of H2 gas are produced.
The enthalpy of the decomposition reaction of N2H4 gas is exothermic, meaning that it releases heat energy into the surroundings. This is because the products (N2 and H2) have a lower enthalpy than the reactant (N2H4).
The enthalpy of the decomposition reaction of N2H4 gas can be affected by factors such as temperature, pressure, and the presence of catalysts. A higher temperature can increase the rate of reaction and result in a larger enthalpy change.
The enthalpy of the decomposition reaction of N2H4 gas can be experimentally determined using calorimetry. This involves measuring the temperature change of the reaction mixture and using it to calculate the enthalpy change. The experimental value can then be compared to the theoretical value calculated using thermodynamic data.