A chemist wishes to perform the following reaction: N₂ + 3 H₂ → 2 NH₃ If only 14.0 g of N₂ is available,what is the minimum amount,in grams,of H₂ needed to completely react with this quantity of N₂?

Question

Quizplus · Accepted Answer

To determine the minimum amount of H₂ needed to completely react with 14.0 g of N₂, we need to use stoichiometry. First, we need to balance the equation: N₂ + 3 H₂ → 2 NH₃ From the balanced equation, we can see that we need 3 moles of H₂ for every mole of N₂. We can use the molar mass of N₂ to find the number of moles available: 14.0 g N₂ x (1 mole N₂ / molar mass N₂) = 0.0684 moles N₂ To completely react with 0.0684 moles of N₂, we need: 0.0684 moles N₂ x (3 moles H₂ / 1 mole N₂) = 0.2052 moles H₂ Finally, we can use the molar mass of H₂ to find the minimum amount needed in grams: 0.2052 moles H₂ x (molar mass H₂ / 1 mole H₂) = 3.03 g H₂ Therefore, the minimum amount, in grams, of H₂ needed to completely react with 14.0 g of N₂ is 3.03 g. The answer is (C).

A Chemist Wishes to Perform the Following Reaction: N2

A Chemist Wishes to Perform the Following Reaction: N₂