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Nitrogen N2 gas and hydrogen H2 gas react to form ammonia NH3gas. Suppose you have11.0molofN2and5.0molofH2in a reactor. Suppose as much as possible of theN2 reacts. How much will be left? Round your answer to the nearest 0.1 mol.

Question

Nitrogen

 N2 

gas

 

and hydrogen

 H2 

gas react to form ammonia

 NH3

gas. Suppose you have

11.0
mol

of

N2

and

5.0
mol

of

H2

in a reactor.

 

Suppose as much as possible of the

N2

 reacts. How much will be left? Round your answer to the nearest 

0.1

 

mol

.

check_circleAnswer
Step 1

The balanced equation for the reaction of formation of ammonia can be given as

N, (g)+3H,(g)2NH, (g)
1mole of N, reactswith 3moles of H
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N, (g)+3H,(g)2NH, (g) 1mole of N, reactswith 3moles of H

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Step 2

From the given moles of reactants, mass is calculated and with each reactant the number of moles of ammonia formed can be calculated.

Given,N 11.0mol
H2 5.0mo
massof N
mass-molesxmolar mass
= 11.0molx14 g/mol
=154 gN
massof H
-5.0molx2g/mol
=10.0gH
Molesof NH, formedfrom N
=11.0mol N x2molNH,
mol N
22.0molNH
Molesof NH, formedfromH2
5.0molHmol NH3
3 mol H
2
3.33mol NH
The excess reactant is N, andlimitingreactantis H
help_outline

Image Transcriptionclose

Given,N 11.0mol H2 5.0mo massof N mass-molesxmolar mass = 11.0molx14 g/mol =154 gN massof H -5.0molx2g/mol =10.0gH Molesof NH, formedfrom N =11.0mol N x2molNH, mol N 22.0molNH Molesof NH, formedfromH2 5.0molHmol NH3 3 mol H 2 3.33mol NH The excess reactant is N, andlimitingreactantis H

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Step 3

The mass of excess reactant that is used up ...

massof excess reactant usedup:
5.0HImoIN,
-50H2 3molH
-1.66molN
1.66molN14gN
1mol
-23.3gN
help_outline

Image Transcriptionclose

massof excess reactant usedup: 5.0HImoIN, -50H2 3molH -1.66molN 1.66molN14gN 1mol -23.3gN

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