How much dihydrogen will be required to reduce completely a #1.22*mol# quantity of dinitrogen gas?

Answer 1

#1/2N_2(g) + 3/2H_2(g) rarr NH_3(g)#

Given the stoichiometry, precisely #3.66*mol# dihydrogen gas are required to give ammonia. Each equiv dinitrogen requires three equiv dihydrogen. How much ammonia gas would be produced given complete reaction (an unlikely scenario)?

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Answer 2

Cameron Andrews

To completely reduce 1.22 moles of dinitrogen gas (N2), you need an equal amount of dihydrogen gas (H2) according to the balanced chemical equation:

N2 + 3H2 → 2NH3

This equation shows that one mole of N2 reacts with three moles of H2 to produce two moles of NH3. Therefore, you would need 3.66 moles of dihydrogen gas (H2) to completely reduce 1.22 moles of dinitrogen gas (N2).

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.