Diborane is produced when hydrogen gas reacts with boron as shown by the chemical equation below. 2B(s)+3H_(2)(g)arrow B_(2)H_(6)(g) If 8.48 mol hydrogen gas is added to a reaction container with 5.88 mol boron, which statement is true? The limiting reagent depends on the amount of diborane produced. Hydrogen gas is the limiting reagent. Boron is the limiting reagent. Both reactants will react completely.

To determine the limiting reagent, we need to compare the mole ratio of the reactants with the coefficients in the balanced chemical equation.<br /><br />The balanced equation is:<br />\[ 2B(s) + 3H_2(g) \rightarrow B_2H_6(g) \]<br /><br />From the equation, 2 moles of boron react with 3 moles of hydrogen gas. <br /><br />First, let's find out how many moles of boron are needed to react with 8.48 moles of hydrogen gas:<br />\[ \text{Moles of B} = \frac{2}{3} \times 8.48 = 5.65 \text{ moles of B} \]<br /><br />We have 5.88 moles of boron available, which is more than the 5.65 moles required. Therefore, hydrogen gas will be completely consumed first.<br /><br />Now, let's check how many moles of hydrogen gas are needed to react with 5.88 moles of boron:<br />\[ \text{Moles of H}_2 = \frac{3}{2} \times 5.88 = 8.82 \text{ moles of H}_2 \]<br /><br />We only have 8.48 moles of hydrogen gas available, which is less than the 8.82 moles required. Therefore, hydrogen gas is the limiting reagent.<br /><br />Thus, the correct statement is:<br />Hydrogen gas is the limiting reagent.