3H2(g)+N2(g)→2NH3(g) 1.36 g H2 is allowed to react with 9.51 g N2, producing 1.06 g NH3 1.) What is the theoretical yield in grams for this reaction under the given conditions? 2.)What is the percent yield for this reaction under the given conditions?

Explanation:

Hello,

In this case, given the chemical reaction and the initial amounts, we first identify the limiting reactant by verifying the reactant yielding the smallest amount of product:

Thus, since the hydrogen yields the least amount of ammonia, it is the limiting reactant, which means the theoretical yield of ammonia is:

Finally, the percent yield for a 1.06-g actually yielded amount turns out:

Best regards.

2b2t

explanation:

2b2t