Answer:
<em>249 kJ</em>
Explanation:
To obtain the energy change of the reaction:
H₂O → H₂ + ¹/₂ O₂
It is necessary to obtain the difference between bond energy of the products and bond energy of the reactant, thus:
Energy of products:
1 mol of H-H bond × 436 kJ/mol = 436 kJ
¹/₂ mol of O=O bond × 498 kJ/mol = 249 kJ
Energy of reactant:
2 mol of H-O bond × 467 kJ/mol = 934 kJ
Energy change of the reaction is:
934 kJ - (436 kJ + 249 kJ) = <em>249 kJ</em>
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I hope it helps!
Answer:
carbon nitrogen and oxygen
im just answering questions to get points Explanation:
i dont know what points do
Moles(AL)/moles(CL2) = 2/3
moles(CL2) = 3/2 * 3.90
moles(CL2) = 5.85 mol
The final volume of the nitrogen sample would be 790 mL
<h3>Charle's Law</h3>
According to Charles, at constant pressure, the volume of a gas is directly proportional to its temperature.
Mathematically: v1/t1 = v2/t2, where v1 and v2 = initial and final volume, and t1 and t2 = initial and final temperature.
In this case, t1 = 37 °C or 310 K, t2 = 77 °C or 350 K, v1 = 700 mL
Thus: v2 = v1 x t2/t1 = 700 x 350/310 = 790 mL
More on Charle's law can be found here: brainly.com/question/16927784
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