How many grams of N₂H₄ are produced from the reaction of 2.0 g of H₂ witH₂ 8 g of N₂ as shown in the following balanced equation?
2 H₂ + N₂→N₂H₄

Question

How many grams of N₂H₄ are produced from the reaction of 2.0 g of H₂ witH₂ 8 g of N₂ as shown in the following balanced equation? 2 H₂ + N₂→N₂H₄

Quizplus · Accepted Answer

To determine the amount of N₂H₄ produced, we need to use stoichiometry. From the balanced equation, we can see that 2 moles of H₂ reacts with 1 mole of N₂ to produce 1 mole of N₂H₄. First, we need to convert the mass of H₂ to moles: 2.0 g H₂ x (1 mol H₂/32.06 g H₂) = 0.0624 mol H₂ Next, we need to convert the mass of N₂ to moles: 8.0 g N₂ x (1 mol N₂/184.12 g N₂) = 0.0434 mol N₂ Since we have more moles of H₂ than N₂, H₂ is the limiting reactant. This means that all of the H₂ will be consumed in the reaction and the amount of N₂H₄ produced will be determined by the amount of H₂ present. Using the mole ratio from the balanced equation, we can calculate the moles of N₂H₄ produced: 0.0624 mol H₂ x (1 mol N₂H₄/2 mol H₂) = 0.0312 mol N₂H₄ Finally, we can convert the moles of N₂H₄ to grams: 0.0312 mol N₂H₄ x (358.4 g N₂H₄/1 mol N₂H₄) = 11.2 g N₂H₄ Therefore, the answer is B) 16 g.

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