Tin metal reacts with hydrogen fluoride to produce tin(II) fluoride and hydrogen gas according to the following balanced equation.
Sn(s)+2HF(g)→SnF2(s)+H2(g)
Sn(s)+2HF(g)→
SnF
2
(s)+
H
2
(g)
How many moles of hydrogen fluoride are required to react completely with 75.0 g of tin?
Step 1: List the known quantities and plan the problem.
Known
given: 75.0 g Sn
molar mass of Sn = 118.69 g/mol
1 mol Sn = 2 mol HF (mole ratio)
Unknown
mol HF
Use the molar mass of Sn to convert the grams of Sn to moles. Then use the mole ratio to convert from mol Sn to mol HF. This will be done in a single two-step calculation.
g Sn → mol Sn → mol HF
Step 2: Solve.
75.0 g Sn×1 mol Sn118.69 g Sn×2 mol HF1 mol Sn=1.26 mol HF
75.0 g Sn×
1
mol Sn
118.69
g Sn
×
2
mol HF
1
mol Sn
=1.26 mol HF
Step 3: Think about your result.
The mass of tin is less than one mole, but the 1:2 ratio means that more than one mole of HF is required for the reaction. The answer has three significant figures because the given mass has three significant figures.
I think it’s “number” and “type”
0.20 moles of iron will be formed in the reaction.
Explanation:
The balanced chemical equation for the reaction between iron (iii) oxide and carbon monoxide to form Fe is to be known first.
the balanced reaction is :
Fe2O3 + 3CO⇒ 2 Fe + 3 CO2
so from the data given the number of moles of carbon monoxide can be known:
3 moles of CO reacted with Fe2O3 to form 2 moles of iron in the reaction.
Number of moles of CO is 6.20 moles
11.6 gm of iron is formed
so the number of moles of iron formed is calculated as
n = mass of iron ÷ atomic weight of iron
= 11.6 ÷ 55.84
= 0.20 moles of iron will be formed when 11.6 gram of iron is produced.
Answer:
Explanation:
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Answer:
For example, in a molecule of aspirin, C9H8O4, there are 9 carbon atoms, 8 hydrogen atoms and 4 oxygen atoms. compound.
Explanation:
