Given the reaction: 4 NH3(g) + 5 O2(g) → 4 NO (g) + 6 H2O When 1.20 mole of ammonia reacts, how many moles of water are produced
1 answer:
Answer:
When 1.20 mole of ammonia reacts, 1.8 moles of water are produced.
Explanation:
The balanced reaction is:
4 NH₃(g) + 5 O₂(g) → 4 NO (g) + 6 H₂O
By stoichiometry of the reaction, the following amounts of moles participate in the reaction:
- NH₃: 4 moles
- O₂: 5 moles
- NO: 4 moles
- H₂O: 6 moles
Then you can apply the following rule of three: if by stoichiometry 4 moles of ammonia produce 6 moles of water, 1.2 moles of ammonia will produce how many moles of water?
moles of water= 1.8 moles
<u><em>When 1.20 mole of ammonia reacts, 1.8 moles of water are produced.</em></u>
<u><em></em></u>
You might be interested in
<u>Answer </u>
Answer 1 : 28.9 g of CO is needed.
Answer 2 : Six moles of over Nine moles of
Answer 3 : Four over two fraction can be used for the mole ratio to determine the mass of Fe from a known mass of .
Answer 4 : Mass of = (150 × 3 × 31.998) ÷ (232.29 × 1) grams
Answer 5 : 8.4 moles of sodium cyanide (NaCN) would be needed.
<u>Solution </u>
Solution 1 : Given,
Given mass of = 55 g
Molar mass of = 159.69 g/mole
Molar mass of CO = 28.01 g/mole
Moles of =
=
= 0.344 moles
Balanced chemical reaction is,
From the given reaction, we conclude that
1 mole of gives → 3 moles of CO
0.344 moles of gives → 3 × 0.344 moles of CO
= 1.032 moles
Mass of CO = Number of moles of CO × Molar mass of CO
= 1.032 × 28.01
= 28.90 g
Solution 2 : The balanced chemical reaction is,
From the given reaction, we conclude that the Six moles of over Nine moles of
is the correct option.
Solution 3 : The balanced chemical reaction is,
From the given balanced reaction, we conclude that Four over two fraction can be used for the mole ratio to determine the mass of Fe from a known mass of .
Solution 4 : Given,
Given mass of = 150 g
Molar mass of = 232.29 g/mole
Molar mass of = 31.998 g/mole
Moles of =
=
The balanced chemical equation is,
From the given balanced equation, we conclude that
1 mole of gives → 3 moles of
of
gives →
of
Mass of = Number of moles of
× Molar mass of
=
Therefore, the mass of = (150 × 3 × 31.998) ÷ (232.29 × 1) grams
Solution 5 : Given,
Number of moles of = 4.2 moles
Balanced chemical equation is,
From the given chemical reaction, we conclude that
1 mole of obtained from 2 moles of NaCN
4.2 moles of obtained → 2 × 4.2 moles of NaCN
Therefore,
The moles of NaCN needed = 2 × 4.2 = 8.4 moles