Lighting a match changes chemical energy into heat.
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The grams of aluminium extracted from 5000g of alumina is 2647 grams
<h3>Chemical formula of alumina:</h3>
Let's calculate the molecular mass of Al₂O₃
Al₂O₃ = 27 × 2 + 16 × 3 = 54 + 48 = 102 g/mol
Therefore,
102 g of Al₂O₃ = 54 g of aluminium
5000g of Al₂O₃ = ?
mass of aluminium produced = 5000 × 54 / 102
mass of aluminium produced = 270000 / 102
mass of aluminium produced = 2647.05882353
mass of aluminium produced = 2647 grams
learn more on mass here: brainly.com/question/14627327
<span>If heat is consumed during a reaction, the reaction is said to be an endothermic reaction.
There are two types of reactions related to heat energy, these are endothermic and exothermic </span>reactions.
Exothermic reactions are when the reactions as it proceeds gives out heat energy to the surroundings. Endothermic reactions are when heat energy is absorbed by the reactants to initiate and continue the reaction. Therefore reaction system absorbs or consumes heat energy from the surrounding.
Answer:
(a) ![BaCl_2(aq)+Na_2SO_4(aq)\rightarrow BaSO_4(s)+2NaCl(aq)](https://tex.z-dn.net/?f=BaCl_2%28aq%29%2BNa_2SO_4%28aq%29%5Crightarrow%20BaSO_4%28s%29%2B2NaCl%28aq%29)
(b) The particles of the formed barium sulfate remain suspended in the aqueous media forming a colloid.
Explanation:
Hello,
In this case, when solutions of barium chloride and sodium sulfate are mixed, the following chemical reaction is carried out:
![BaCl_2(aq)+Na_2SO_4(aq)\rightarrow BaSO_4(s)+2NaCl(aq)](https://tex.z-dn.net/?f=BaCl_2%28aq%29%2BNa_2SO_4%28aq%29%5Crightarrow%20BaSO_4%28s%29%2B2NaCl%28aq%29)
Thus, we can notice that the product barium sulfate remains solid since its solubility in aqueous media is very low, for that reason at the beginning the solution becomes cloudy as its particles remain suspended in the water forming a colloid. Nevertheless, after some days, the suspended particles get precipitated by the effect of the gravity, therefore, we observe the solid on the bottom of the beaker.
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The amount of heat required to melt 15.0 grams of ice at 0.0º C is<u> 4950 J.</u>
<h3>What is the amount of heat required to melt 15.0 grams of ice at 0.0º C?</h3>
The amount of heat required to melt 15.0 grams of ice at 0.0º C is calculated from the formula given below:
Amount of heat = mass * latent heat of fusion of ice
The latent heat of fusion is the amount of heat required to convert a unit mass of ice at 0.0º C to water at 0.0º C
The latent heat of fusion of ice is 330J/g
mass of ice = 15.0 g
Amount of heat required = 15.0 g * 330 J/g
Amount of heat required = 4950 J
Learn more about latent heat of fusion at: brainly.com/question/87248
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