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kenny6666 [7]
3 years ago
9

How does the separation of a mixture containing salt, sand and naphthalene support the law of conservation of matter

Chemistry
1 answer:
Elis [28]3 years ago
3 0

Answer:

Mixtures are not unique to chemistry; we encounter them on a daily basis. The food and drinks ... The mixture that will be separated in this experiment contains three components: Naphthalene ... Dissolving the table salt with water to extract it from the sand by filtration, and. 3. ... support the Law of Conservation of Matter.

Explanation:

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Observation or inference<br> The container is filled to the 350 ml mark with water
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Observation is acknowledging and noting some facts from the surroundings or the environment. Usually, observation is done using the five senses of human such as the sense of sight, sense of smell, sense of touch, sense of hearing and sense of tasting. It can also be qualitative and quantitative. Qualitative observations are those who use non-numeric forms in expressing the observation however quantitative uses numeric forms in presenting the observation. Inference on the other hand is the probable explanation or interpretation based on the observation given. Therefore, the statement "The container is filled to the 350 ml mark with water " is an observation.
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How are physical and<br>chemical changes different?​
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Does H₂ have a coefficient?
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Reaction enthalpy for ethanol oxidation, C2H5OH+3O2 -&gt; 2CO2 + 3H2O is 1257 kJ/mole. Energy content per mol fuel ______kJ Ener
MArishka [77]

Answer:

Energy content per mol fuel 1257 kJ.

Energy content per gram fuel = 27.33  kJ

Energy released per mol carbon dioxide gas formed is 628.5 kJ

Energy released per mol oxygen gas consumed= 419 kJ

Moles of carbon dioxide gas formed per 1000 kJ energy released is 1.591.

Explanation:

C_2H_5OH+3O_2\rightarrow 2CO_2 + 3H_2O,\Delta H= 1257 kJ/mol

1) Energy released per mole or fuel that is ethanol :

1mol \times 1257 kJ/mol=1257 kJ

2) Mass of 1 mole of ethanol = 46 g

46 grams of ethanol produces 1257 kJ of energy

Energy content per gram fuel :

\frac{1257 kJ}{46 g}=27.33 kJ/g

3) Energy released when 2 moles of carbon dioxide are formed = 1257 kJ

Energy released per mol of carbon dioxide formed:

\frac{1}{2}\times 1257 kJ/mol=628.5 kJ/mol

4) Energy released when 3 moles of oxygen gas are consumed = 1257 kJ

Energy released per mol of oxygen gas consumed:

\frac{1}{3}\times 1257 kJ/mol=419 kJ/mol

5) Energy released when 2 moles of carbon dioxide are formed = 1257 kJ

Moles of carbon dioxide gas formed per kilo Joule of energy:

\frac{2}{1257} mol

Moles of carbon dioxide gas formed when 1000 kJ of heat is released:

\frac{2}{1257} \times 1000 mol=1.591 mol

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