0.050 mols \( \mathrm{N} \times \frac{2}{1} \) mols H

Did you know that nitrogen (N) and hydrogen (H) are essential components in the formation of ammonia (NH₃), which is crucial for fertilizers? In fact, the Haber process, developed in the early 20th century, is a method for synthesizing ammonia from these two gases. This significant industrial process transformed agriculture and has helped feed billions of people around the world! When calculating mols of hydrogen from nitrogen, it's important to keep in mind the stoichiometry of the reaction. For every mole of nitrogen, two moles of hydrogen are required. So, when you calculate \(0.050 \, \text{mol N} \times \frac{2 \, \text{mol H}}{1 \, \text{mol N}}\), you get \(0.100 \, \text{mol H}\). A common mistake is forgetting to balance the equation, which can lead to incorrect molar ratios. Always double-check your stoichiometric coefficients!