(i) According to Avogadro's law, at constant temperature and pressure, equal volumes of gases contain equal numbers of moles. Therefore, the volumes of the reactant gases (N2 and H2) and the product gas (NH3) will be in a simple ratio of their coefficients in the balanced chemical equation.
(ii) The balanced chemical equation for the formation of ammonia from nitrogen and hydrogen is:
N2 + 3H2 → 2NH3
Since the stoichiometric coefficient of NH3 is 2, for every one mole of N2 reacted, two moles of NH3 are produced. So, if the reaction goes to completion, 1.00 mole of N2 will produce 2.00 moles of NH3.
(iii) To calculate the volume of ammonia gas produced, we use Avogadro's law, which states that equal volumes of gases at the same temperature and pressure contain equal numbers of moles. Given that 1 mole of N2 produces 2 moles of NH3, and the initial volume of the reactant gases is not specified, we cannot directly calculate the volume of NH3 produced without additional information.
(iv) Avogadro's law is applied in this scenario to determine the relationship between the volumes of gases involved in the reaction and the number of moles of each gas present. It helps us understand how the volume of gases changes with the number of moles of gas molecules present, given constant temperature and pressure.
(v) Avogadro's law has several practical implications in chemical reactions. It allows chemists to predict the volumes of reactant gases required for a reaction, the volumes of product gases produced, and to scale up reactions from laboratory to industrial scales. Additionally, it provides a basis for stoichiometric calculations, enabling precise control over reaction conditions and product yields.
