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Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2(g)+3H2(g)--->2NH3(g).

A ______g sample of N2 requires 3.0 g of H2 for complete reaction.

a)0.76

b)1.2

c)14.0

d)17.2

Respuesta :

joseaaronlara

Answer:

The answer to your question is:        14 g of N₂

Explanation:

Data

MW N2 = 14

MW H2 = 1

MW NH3 = 17

                                  N₂(g)  +   3H₂(g)    --->   2NH₃(g).

                                 28g           6g                  34g

               

                             28 g of N₂ --------------------  6 g of H₂

                               x              --------------------  3 g of H₂

                               x = (3 x 28) / 6

                               x = 14 g of N₂

                               

A 14gram sample of Nâ‚‚ requires 3.0 g of Hâ‚‚ for complete reaction.

How we calculate mass from moles?

Mass of any substance will be calculated from its moles as:

n = W/M, where

W = required mass

M = molar mass

Given chemical reaction is:

N₂(g)+3H₂(g) → 2NH₃(g)

Moles of 3 gram of Hâ‚‚ = 3

From the stoichiometry of the reaction, it is clear that

1 mole of Nâ‚‚ = react with 3 mole of Hâ‚‚

Mass of 1 mole of Nâ‚‚ = 14 grams

Hence, 14 grams of nitrogen is required.

To know more about moles, visit the below link:

https://brainly.com/question/13860160


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