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Considering the definition of molar mass, the moles of gas used are 10.625 moles.
<h3>Definition of molar mass</h3>The molar mass of substance is a property defined as its mass per unit quantity of substance, in other words, molar mass is the amount of mass that a substance contains in one mole.
<h3>Amount of moles used</h3>Natural gas has a molar mass of 16.0 g/mole.
You started out the day with a tank containing 200.0 g of natural gas. So, you can apply the following rule of three: If by definition of molar mass 16 grams are contained in 1 mole, 200 grams are contained in how many moles?
<u><em>amount of moles at the beginning= 12.5 moles</em></u>
At the end of the day, your tank contains 30.0 g of natural gas. So, you can apply the following rule of three: If by definition of molar mass 16 grams are contained in 1 mole, 30 grams are contained in how many moles?
<u><em>amount of moles at the end= 1.875 moles</em></u>
The number of moles used will be the difference between the number of moles used initially and the contents at the end of the day.
moles used= amount of moles at the beginning - amount of moles at the end
moles used= 12.5 moles - 1.875 moles
<u><em>moles used= 10.625 moles</em></u>
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Finally, the moles of gas used are 10.625 moles.
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Explanation:
Let us assume that the volume of given aqueous solution is 7.5 L.
Therefore, according to Henry's law, the relation between concentration and pressure is as follows.
C =
where, pressure (P) = 760 torr = 1 atm
According to Henry's law, constants for gases in water at are as follows.
= 0.21 atm = 0.21 bar
= 0.78 atm = 0.78 bar
for
=
for
=
Since, 21% oxygen is present in air so, its mass will be 0.21 g. Similarly, 78% nitrogen means the mass of nitrogen is 0.78 g.
Therefore, concebtrations will be calculated as follows.
Now, we will calculate the number of moles as follows.
mol
mol
As the molar mass of = 32 g/mol
Hence, mass of oxygen will be as follows.
Mass of
= 63.84 mg
As the molar mass of = 28
Mass of = 102.5 mg
Thus, we can conclude that mass of oxygen is 63.84 mg and nitrogen is 102.5 mg.
Answer: The empirical formula is and molecular formula is
Explanation:
We are given:
Mass of = 18.95 g
Mass of = 7.759 g
Molar mass of carbon dioxide = 44 g/mol
Molar mass of water = 18 g/mol
For calculating the mass of carbon:
In 44g of carbon dioxide, 12 g of carbon is contained.
So, in 18.59 g of carbon dioxide, = of carbon will be contained.
For calculating the mass of hydrogen:
In 18g of water, 2 g of hydrogen is contained.
So, in 7.759 g of water, = of hydrogen will be contained.
Mass of C = 5.07 g
Mass of H = 0.862 g
Step 1 : convert given masses into moles.
Moles of C =
Moles of H=
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For C =
For H =
The ratio of C : H = 1: 2
Hence the empirical formula is .
The empirical weight of = 1(12)+2(1)= 14 g.
The molecular weight = 56.1 g/mole
Now we have to calculate the molecular formula.
The molecular formula will be=