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hydrogen cyanide is prepared from ammonia , air and natural gas if a reaction vessel contains 51 gm of NH3 what is the maximum amount of HCN that could be made assuming the reaction goes to completion and what volumes of O2 and CH4 gases required for the reaction at STP
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Asked on December 20, 2019 by
Archit Yasmin
Hydrogen cyanide, HCN, is prepared from ammonia, air and natural gas (CH
4
) by the following process.
2NH
3
(g)+3O
2
(g)+2CH
4
(g)
Pt
2HCN(g)+6H
2
O(g)
If a reaction vessel contains 11.5gNH
3
,10.0gO
2
and 10.5gCH
4
, what is the maximum mass, in grams, of hydrogen cyanide that could be made, assuming the reaction goes to completion?
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ANSWER
NH
3
+3O
2
+2CH
4
→2HCN+6H
2
O
given 11.5 10 10.5
moles
17
11.5
32
10
16
10.5
⇒0.67 0.31 0.656
stoichiometry
2
0.67
3
0.31
2
0.656
0.335 0.103 0.328
↓
limiting
3 moles O
2
→2 moles HCN
0.31 mole O
2
→x mole HCN
x=
3
2×0.31
=0.206
moles of HCN=0.206
mass of HCN=0.206×[1+12+14]
=5.562 gm
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Explanation:
ANSWER
NH3+3O2+2CH4→2HCN+6H2O
given 11.5 10 10.5
moles 1711.5 3210 1610.5
⇒0.67 0.31 0.656
stoichiometry 20.67 30.31 20.656
0.335 0.103 0.328
↓
limiting
3 moles O2→2 moles HCN
0.31 mole O2→x mole HCN
x=32×0.31=0.206
moles of HCN=0.206
mass of HCN=0.206×[1+12+14]
=5.562 gm
Option B is answer
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