Question

if 75 moles of ammonia is needed, how many grams of nitrogen will be consumed? N2(g) + 3H2(g) --> 2NH3(g)

Answer 1

Answer:

Amount of nitrogen consumed comes out to be 1050 g

Explanation:

Number of moles of ammonia needed = 75 mole

The balanced reaction is shown below

$\textrm{N}_{2}\left ( g \right )+3\textrm{H}_{2}\left ( g \right )\rightarrow 2\textrm{NH}_{3}\left ( g \right )$

1 mole of ammonia is needed for producing 2 mole ammonia according to the balanced reaction.

Number of moles of nitrogen needed for producing 75 mole ammonia = 37.5 mole

Molar mass of nitrogen gas = 28 g/mole

Amount of nitrogen gas needed = $\left ( 37.5 \textrm{ mole}\times 28 \textrm{ g/mol} \right ) = 1050 \textrm{ g}$

Amount of nitrogen gas needed = 1050 g

Answer 2

Answer: 37.5

Explanation: Since NH3 has a coefficient of 2, that means it will produce 2x the moles as N2. Since 75 moles of NH3 will be used, in order to figure out N2 you would do the following:

75 mol / 2 = 37.5

Oh wait this said grams, sorry! Let me fix it.