A molecule has the empirical formula C4H6O. If its molecular weight is determined to be about 212 g/mol, what is the most likely
2 answers:
Answer:
The molecular formula is most likely to be first option, .
Explanation:
Both the molecular formula and the empirical formula of a molecule give the types of atoms in that molecule. However, the molecular formula of a molecule gives the exact number of atoms each molecule. On the other hand, the empirical formula gives only a simplified ratio.
For example, if the empirical formula of the molecule is , then the molecular formula would be
, or equivalently
, where
is a positive whole number (
, etc.) The goal here is to find the value of
Look up the relative atomic mass data on a modern periodic table:
- C: 12.011.
- H: 1.008.
- O: 15.999.
The formula mass of would be
.
The formula mass of would be
.
On the other hand, since the molecule should have a molecular mass of ,
.
. (Round to the nearest whole number.)
Hence, the molecular formula would be , which simplifies to
.
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Answer:
The answer is "Option B"
Explanation:
From the query, the following knowledge is derived:
Yield in percentage = 47%
Performance of theory = 4860 g
Actual yield Rate =?
The percentage return is defined simply by the ratio between both the real return as well as the conceptual return multiplied by the 100. It's also represented as numerically:
Now We can obtain the percent yield as followed using the above formula:
The value of the Actual yield Rate =
The Actual yield Rate= 2284.2 g.
Answer:
Value of equilibrium constant is 0.0888
Explanation:
Both and
are gaseous. Hence equilibrium constant depends upon partial pressures of
and
.
Initially no and
were present.
Hence mole fraction of and
at equilibrium can be calculated from coefficient of
and
in balanced equation.
Mole fraction of = (number of moles of
)/(total number of moles of
and
) =
Mole fraction of = (number of moles of
)/(total number of moles of
and
) =
Let's assume both and
behaves ideally.
Therefore partial pressure of ,
and P_{CO_{2}}= x_{CO_{2}}.P_{total}
Where x represents mole fraction
So,
So,