#N_2 + 3H_2 -> 2NH_3#. What is the limiting reactant if you start the reaction with 10.0 moles of each reactant?

Answer 1

#H_2#

The reaction equation says that three moles of #H_2# and one mole of #N_2# are required to make two moles of ammonia. Since more #H_2# is used up per mole #NH_3# produced, the hydrogen will be used up first.

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Answer 2

Peyton Adams

#H_2 ."is". the. "limiting". "reactant"#

A quick way to determine limiting reagent (or, reactant) is to convert all data dimensions to moles and divide each by the respective coefficient in the balanced Equation. The smaller number will be the limiting reactant.

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Answer 3

Mateo Aguilar

The limiting reactant is N2, as it requires more moles of H2 than are available for complete reaction, leading to the exhaustion of H2 before all of the N2 reacts.

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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.

#N_2 + 3H_2 -&gt; 2NH_3#. What is the limiting reactant if you start the reaction with 10.0 moles of each reactant?

#N_2 + 3H_2 -> 2NH_3#. What is the limiting reactant if you start the reaction with 10.0 moles of each reactant?