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maxonik [38]
3 years ago
11

0.2 mol of hydrocarbons undergo complete combustion to give 35.2 of carbon dioxide and 14.4g of water as the only product. What

is the molecular formula of hydrocarbon
Chemistry
1 answer:
MaRussiya [10]3 years ago
6 0

Answer:

\rm C_4 H_8.

Explanation:

Look up the relative atomic mass of \rm C, \rm H, and \rm O on a modern periodic table:

  • \rm C: 12.011.
  • \rm H: 1.008.
  • \rm O: 15.999.

Calculate the molecular mass of \rm CO_2 and \rm H_2O:

M(\mathrm{CO_2}) = 12.011 + 2 \times 15.999 = 44.009\; \rm g \cdot mol^{-1};

M(\mathrm{H_2O}) = 2 \times 1.008 + 15.999 = 18.015\; \rm g \cdot mol^{-1}.

Given the mass m of \rm CO_2 and \rm H_2O produced, calculate the number of moles of molecules that were produced:

\displaystyle n(\mathrm{CO_2}) = \frac{m(\mathrm{CO_2})}{M(\mathrm{CO_2})} \approx 0.80\; \rm mol;

\displaystyle n(\mathrm{H_2O}) = \frac{m(\mathrm{H_2O})}{M(\mathrm{H_2O})} \approx 0.80\; \rm mol.

Calculate the number of moles of \rm C atoms and \rm H atoms in these \rm CO_2 and \rm H_2O molecules.

  • Each \rm CO_2 molecule contains one \rm C atom. Therefore, that 0.80\; \rm mol of \rm CO_2\! contains 0.80\; \rm mol\! of \rm C\! atoms.
  • Each \rm H_2O molecule contains two \rm H atoms. Therefore, that 0.80\; \rm mol of \rm H_2O\! contains 2 \times 0.80\; \rm mol = 1.60\; \rm mol of \rm H\! atoms.

The combustion reaction here include two reactants: the hydrocarbon and \rm O_2.

As the name suggests, hydrocarbons contain only \rm C atoms and \rm H atoms. On the other hand, \rm O_2 contains only \rm O atoms.

Therefore, all the \rm C and \rm H atoms in those \rm CO_2 and \rm H_2O molecules are from the unknown hydrocarbon. (With a similar logic, all the \rm O atoms in those combustion products are from \rm O_2.)

In other words, that 0.20\; \rm mol of this unknown hydrocarbon molecules contains:

  • 0.80\; \rm mol of \rm C atoms, and
  • 1.60\; \rm mol of \rm H atoms.

Hence, each of these hydrocarbon molecules would contain (0.80\; \rm mol) / (0.20\; \rm mol) = 4 carbon atoms and (1.60\; \rm mol) / (0.20\; \rm mol) = 8 hydrogen atoms.

The molecular formula of this hydrocarbon would be \rm C_{4} H_{8}.

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Otrada [13]

Answer:

Uranium must be purified before it is used as a fuel source

Explanation:

The purer the uranium sample, the more the concentration of uranium in the fuel is.

Whenever uranium is extracted from nature, it contains a lot of impurities. Only a few special nuclear reactors can utilize uranium in this raw state. most of the others have to get uranium to become about 3% pure before they begin using it.

To do this, uranium has to be passed through a series of chemical reactions all with the aim of extracting the other compounds that may be present in the fuel.

5 0
2 years ago
Bond length is the distance between the centers of two bonded atoms. On the potential energy curve, the bond length is the inter
mariarad [96]

Answer:

152 pm

Explanation:

According to the question, we can estimate the bond length from the given values of the atomic radii. This now is the upper limit of the bond length for the molecule.

Since we have that;

Atomic radius of H= 37.0 pm

Atomic radius of Br = 115.0 pm

Bond length = Atomic radius of H + Atomic radius of Br

Bond length = 37.0 pm + 115.0 pm

Bond length = 152 pm

5 0
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Name two other than chlorine (CI) that are likely to react with sodium (Na)
agasfer [191]
F and O
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What volume of the stock solution (Part A) would contain the number of moles present in the diluted solution (Part B)?
vova2212 [387]
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6 0
2 years ago
7. Suppose 1.01 g of iron (III) chloride is placed in a 10.00-mL volumetric flask with a bit of water in it. The flask is shaken
Nana76 [90]

<u>Answer:</u> The molarity of Iron (III) chloride is 0.622 M.

<u>Explanation:</u>

Molarity is defined as the number of moles present in one liter of solution.  The equation used to calculate molarity of the solution is:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}

Or,

\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}

We are given:

Mass of iron (III) chloride = 1.01 g

Molar mass of iron (III) chloride = 162.2 g/mol

Volume of the solution = 10 mL

Putting values in above equation, we get:

\text{Molarity of Iron (III) chloride}=\frac{1.01g\times 1000}{162.2g/mol\times 10mL}\\\\\text{Molarity of Iron (III) chloride}=0.622M

Hence, the molarity of Iron (III) chloride is 0.622 M.

3 0
2 years ago
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