The reaction n2 + 3 h2 → 2 nh3 is used to produce ammonia. when 450. g of hydrogen was reacted with nitrogen, 1575 g of ammonia were produced. what is the percent yield of this reaction?

30.8%
61.8%
20.7%
41.5%
more information is needed to solve this problem.

Answer : The percent yield of the reaction is, 61.8 %

Solution : Given,

Mass of = 450 g

Molar mass of = 2 g/mole

Molar mass of = 17 g/mole

First we have to calculate the moles of .

Now we have to calculate the moles of

The balanced chemical reaction is,

From the balanced reaction, we conclude that

As,  3 mole of react to give 2 mole of

So, 225 moles of react to give moles of

Now we have to calculate the mass of

Theoretical yield of = 2550 g

Experimental yield of = 1575 g

Now we have to calculate the percent yield of the reaction.

Therefore, the percent yield of the reaction is, 61.8 %

answer; /// i do believe that the correct answer is (c)nuclear bond

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.