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2 years ago

About 95-98 percent of alcohol is oxidized to what two substances

Chemistry

1 answer:

Sunny_sXe [5.5K]2 years ago

5 0

Answer:

D. Water and Carbondioxide

Explanation:

Combustion of organic compounds in the presence of excess Oxygen will liberate carbondioxide (CO2) and water vapour (H2O). This is an exothermic reaction because heat is liberated to the surroundings.

CnH2n+1OH(aq) + (3/2*n)O2(g) --> nCO2(g) + (n + 1)H2O(g)

Addition of Oxygen can also be termed as a redox reaction. In this case, alcohols are oxidised while the Oxygen is reduced.

Example, (propanol)

C3H7OH(aq) + 9/2O2(g) --> 3CO2(g) + 4H2O(g)

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To dissolve one substance, attractions between solute and solvent particles must be formed, steps involved are:

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A physical process, not a chemical one, takes place when a solute and a solvent combine to produce a solution.
In other words, by applying the right separation techniques, both the solute and the solvent may be recovered in chemically unaltered forms.
It is claimed that two substances are entirely miscible when they combine to create a single homogenous phase in all ratios. Water and ethanol mix well, much like different gas combinations do.
When two substances, like oil and water, are fundamentally insoluble in one another, they are said to be immiscible.
We have already talked about several examples of gaseous solutions, such as the atmosphere of Earth.

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1 year ago

The distance between any two successive places where the shape of the wave repeats itself

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Wave length is the answer.

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2 years ago

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The anticodon is the three-base code on the tRNA molecule that binds to the codon on mRNA. What is the associated codon for the

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Answer:

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Explanation:

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1 year ago

Determine the heat of reaction (ΔHrxn) for the combustion of ethanol (C2H5OH) by using heat of formation data: C2H5OH (l) + 3 O2

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Answer:

$\Delta H_{rxn}=-1234.782kJ$

Explanation:

$\Delta H_{rxn}=\sum [n_{i}\times \Delta H_{f}^{0}(product)_{i}]-\sum [n_{j}\times \Delta H_{f}^{0}(reactant_{j})]$

Where $n_{i}$ and $n_{j}$ are number of moles of product and reactant respectively (equal to their stoichiometric coefficient).

$\Delta H_{f}^{0}$ is standard heat of formation.

So, $\Delta H_{rxn}=[2mol\times \Delta H_{f}^{0}(CO_{2})_{g}]+[3mol\times \Delta H_{f}^{0}(H_{2}O)_{g}]-[1mol\times \Delta H_{f}^{0}(C_{2}H_{5}OH)_{l}]-[3mol\times \Delta H_{f}^{0}(O_{2})_{g}]$

or, $\Delta H_{rxn}=[2mol\times -393.509kJ/mol]+[3mol\times -241.818kJ/mol]-[1mol\times -277.69kJ/mol]-[3mol\times 0kJ/mol]$

or, $\Delta H_{rxn}=-1234.782kJ$

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3 years ago