Given the reaction at 101.3 kilopascals and 298 K:
hydrogen gas +iodine gas →hydrogen iodide gas
This reaction is classified as
(1) endothermic, because heat is absorbed
(2) endothermic, because heat is released
(3) exothermic, because heat is absorbed
(4) exothermic, because heat is released
hydrogen gas +iodine gas →hydrogen iodide gas
This reaction is classified as
(1) endothermic, because heat is absorbed
(2) endothermic, because heat is released
(3) exothermic, because heat is absorbed
(4) exothermic, because heat is released
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The heat of formation of HI(g) is +25.9 kJ/mol, and is therefore endothermic.
That is for this reaction:
1/2 H2(g) + 1/2 I2(s) --> HI(g) .... DH = +25.9 kJ
But your reaction has I2 as a gas, and so some additional energy must be absorbed to vaporize the iodine.
Between the two process, heat must be absorbed, and so the process is endothermic.
That is for this reaction:
1/2 H2(g) + 1/2 I2(s) --> HI(g) .... DH = +25.9 kJ
But your reaction has I2 as a gas, and so some additional energy must be absorbed to vaporize the iodine.
Between the two process, heat must be absorbed, and so the process is endothermic.
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During this reaction a bond is being formed. This most likely means that energy is required to make this reaction go forward, heat being that energy. The correct answer is (1) endothermic, because heat is being absorbed.
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when ever a compound is formed energy is given out