Calculate the volume in milliliters of a 5.55-g sample of a solid with a density of 3.03 g/mL
1 answer:
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Answer:
Explanation:
As we know that
......eq (1)
we will calculate the pH of OH- and then we will calculate the pH of H+
So p[OH-]
Solving the right side of the equation, we get
p[OH-]
Now we know that
Substituting the value of pOH in the above equation, we get -
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=