What is the limiting reagentwhen 150,0 g of nitrogen reacts with 321 g of hydrogen? N_(2)(g)+3H_(2)(g)2NH_(3)(g) There is not a limiting reagent Nitrogen Gas Hydrogen Gas Ammonia

## Step 1<br />The limiting reagent in a chemical reaction is the reactant that is completely consumed first, thus limiting the amount of product that can be formed. In this case, we are given the masses of nitrogen and hydrogen, and we need to determine which one is the limiting reagent.<br /><br />## Step 2<br />First, we need to convert the given masses of nitrogen and hydrogen into moles. The molar mass of nitrogen (N2) is 28.01 g/mol, and the molar mass of hydrogen (H2) is 2.02 g/mol.<br /><br />### **Moles = \(\frac{Mass}{Molar\:Mass}\)**<br /><br />## Step 3<br />Using the formula above, we can calculate the number of moles of nitrogen and hydrogen.<br /><br />## Step 4<br />Next, we compare the number of moles of nitrogen and hydrogen. The stoichiometry of the reaction tells us that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia.<br /><br />## Step 5<br />By comparing the number of moles of nitrogen and hydrogen, we can see that there is more than enough hydrogen to react with all the nitrogen. Therefore, nitrogen is the limiting reagent.