[tex]3H_2+2N_2\rightarrow 2NH_3[/tex]
Given:
The unbalanced chemical equation:
[tex]H_2+N_2\rightarrow NH_3[/tex]
To find:
The balanced chemical equation and to determine of [tex]N_2[/tex] needed to produce 11.35 g of [tex]NH_3[/tex].
Solution:
The balanced chemical reaction:
[tex]3H_2+2N_2\rightarrow 2NH_3[/tex]
Mass of ammonia needed to produce = 11.35 g
Moles of ammonia :
= [tex]\frac{11.35 g}{17.031 g/mol}=0.6664 mol[/tex]
[tex]3H_2+2N_2\rightarrow 2NH_3[/tex]
According to the reaction, 2 moles of ammonia is obtained from 2 moles of dinitrogen, then 0.6664 moles of ammonia will be obtained from :
[tex]=\frac{1}{1}\times 0.6664 mol=0.6664 \text{mol of } N_2[/tex]
Moles of dinitrogen required = 0.6664 mol
Mass of 0.6664 moles of dinitrogen:
[tex]=0.6664 mol\times 28.0134 g/mol=18.67 g[/tex]
The mass of [tex]N_2[/tex] needed is 18.67 grams.
Learn more about the unitary method here:
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