biscmsfmodfibis,/vew.phpi 4121569 Jump to... Ntrogen and hydrogen combine at hig

Question

biscmsfmodfibis,/vew.phpi 4121569 Jump to... Ntrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia. Assume 0.110 mol of N2 and 0.345 mol of H2 are present initially Numbe Afier complete reaction, how moles of ammonia are mol Number mol How many moles of H2 remain? Number How many moles of N2 remain? mol O nitrogen O hydrogen What is the limiting reactant? a Ext oerevous Give up & View Solton Check Answer ONext Hint bout us careers privacy policy terms of use contact us help

Explanation / Answer

1)
Balanced chemical equation is:
N2 + 3 H2 ---> 2 NH3 +


1 mol of N2 reacts with 3 mol of H2
for 0.11 mol of N2, 0.33 mol of H2 is required
But we have 0.345 mol of H2

so, N2 is limiting reagent
we will use N2 in further calculation


Molar mass of NH3,
MM = 1*MM(N) + 3*MM(H)
= 1*14.01 + 3*1.008
= 17.034 g/mol

According to balanced equation
mol of NH3 formed = (2/1)* moles of N2
= (2/1)*0.11
= 0.22 mol
Answer: 0.220 mol

2)
According to balanced equation
mol of H2 reacted = (3/1)* moles of N2
= (3/1)*0.11
= 0.33 mol
mol of H2 remaining = mol initially present - mol reacted
mol of H2 remaining = 0.345 - 0.33
mol of H2 remaining = 0.015 mol
Answer: 0.015 mol

3)
mol of N2 remains = 0 mol because N2 is limiting reagent
Answer: 0 mol

4)
Answer: Nitrogen

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