Answer:
54 g is the theoretical yield
Explanation:
This is the reaction:
2H₂ + O₂ → 2H₂O
So 2 moles of hydrogen react with 1 mol of oxygen, to produce 2 mol of water.
If I have 3 moles of H₂ and 2 moles of O₂, the my limiting reactant is the hydrogen.
1 mol of O₂ react with 2 moles of H₂
S 2 mol of O₂ would react with 4 moles (I only have 3 moles)
Then, ratio is 2:2 the same as 1:1
As 2 mol of H₂ produce 2 moles of water, 3 moles of H₂ will produce 3 moles of H₂O.
This is the theoretical yield in moles. Let's convert them to mass (mol . molar mass)
3 mol . 18g/m = 54 g
Answer:
Explanation:
according to the balance chemical equation
2 moles of c6h14 give us 14 moles of H2O
now mass(in gram) of 2 moles of C6H14 is
moles=mass/molar mass
mass=molar mass*moles
molar mass of C6H14 is 86 therefore
mass=86*2=172
now mass of 14 moles of water is
mass=molar mass*moles
molar mass of water is 18
mass=18*14=252
from the above calculations we conclude that
172 grams of C6H14 produce 252 grams of water
so 1.28 grams of C6H14 produce =252*1.28/172=1.87 grams of water
result is that 1.28 grams of C6H14 produced 1.87 grams of water
Polyatomic ions: , , , , , and
Monatomic ions: , , and
<h3>Monoatomic vs Polyatomic Ions</h3>
In chemistry, monoatomic ions are ions that consist of only a single type of atom. They are usually positive or negatively charged and are otherwise known as simple ions. Examples include , , and
Polyatomic ions, on the other hand, are ions that consist of more than one atom, unlike monoatomic ions. The two or more atoms are covalently bonded and the entire structure behaves like a single chemical entity in reactions. Polyatomic ions are otherwise known as molecular ions.
Examples of polyatomic ions are , , , , , and
Thus, from the diagram:
- Polyatomic ions: , , , , , and
More on ions can be found here: brainly.com/question/14982375
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86.7 kJ
<h3>
Further explanation</h3>
<u>Given:</u>
Molar mass (Mr) of ethanol = 46.07 g/mol
<u>Question:</u>
How much energy is required to vaporize 98.6 g of ethanol (C₂H₅OH) at its boiling point?
<u>The Process:</u>
Observe this . This means that 40.5 kJ of energy is required to vaporize every 1 mole of ethanol at its boiling point. Therefore we must first convert grams into moles.
<u>Question:</u>
Step-1:
Let us count the number of moles of 98.6 g of ethanol.
We obtain 2.14 moles of ethanol.
Step-2:
Let us calculate how much energy is required to vaporize 2.14 moles of ethanol at its boiling point.
The amount of energy required is
Thus, the amount of energy required to vaporize 98.6 g of ethanol at its boiling point is 86.7 kJ.
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Quick Steps
<h3>Learn more</h3>
- Determine the mass of aspirin from the number of molecules brainly.com/question/10567477
- Write the equilibrium constant for the reaction brainly.com/question/10608589
- The chemical problem of mixed concentration brainly.com/question/7596086
Keywords: how much, energy required, to vaporize, ethanol, C₂H₅OH, its boiling point, ΔHvap, molar mass, moles, converts, kJ/mol
Answer:
1935100 Bq
Explanation:
Let us recall that:
If 1 μCi can be equivalent to 37000 Bq
Then; the activity of 52.3 μCi will be: