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Answer:
36 KJ of heat are released when 1.0 mole of HBr is formed.
Explanation:
<em>By Hess law,</em>
<em>The heat of any reaction ΔH for a specific reaction is equal to the sum of the heats of reaction for any set of reactions which in sum are equivalent to the overall reaction:</em>
H 2 (g) + Br 2 (g) → 2HBr (g) ΔH = -72 KJ
This is the energy released when 2 moles of HBr is formed from one mole each of H2 and Br2.
Therefore, Heat released for the formation of 1 mol HBr would be half of this.
Hence,
ΔHreq = -36 kJ
36 KJ of heat are released when 1.0 mole of HBr is formed.
Answer:
O2(g) was Reduced
Explanation:
It is necessary at this point to restate the working definitions of oxidation and reduction.
Oxidation refers to increase in oxidation number. A chemical specie is oxidized in a chemical reaction if there is a positive increase in its oxidation number from left to right in the reaction.
A chemical specie is said to be reduced when there is a decrease in its oxidation number from left to right in a reaction. Hence reduction refers to a decrease in oxidation number.
Now let us focus on O2(g). Its oxidation number on the left hand side is zero. On the right hand side, its oxidation number decreases to -2. This shows a decrease in oxidation number. From our premises above, we can safely conclude that O2(g) was reduced in the reaction.
Answer:
scientific investigation is the quest to find an answer to a question using scientific method.
Explanation:
B and i don’t need to explain it says it there hope it helps
