Respuesta :
Answer: Yes, a given amount of Hydrogen would react with different masses of the two isotopes of chlorine, and no, this does not conflict with the Law of Definite proportions
Explanation:
About 76% percent of Cl is found in the Cl-35 isotope, and about 24% in the Cl.37 isotope. that means that about 24% of Cl nuclei have 2 more neutrons than the average Cl nucleus.
So, if [tex]H_2[/tex] reacts with [tex]Cl_2[/tex], 76% of the Hydrogen that reacted will react with Cl-35, and the rest will react with Cl-37. Why does this not conflict with the law of definite proportions? Because each Hydrogen atom ends up paired to a single Chlorine atom! Moreover, the proportion of Cl-35 to Cl-37 remains constant in all samples of Chlorine that are naturally found, thus we will always find the same proportion of Chlorine to Hydrogen in any HCl sample we come across. Thus the weight of a mol of Cl will always be [tex]35*0.76+37*0.24=35.48[/tex] or 35.45 if we had done this calculation with more significant digits.
Therefore 1 mol of [tex]H_2[/tex] (2 grams) will always react with 1 mol of [tex]Cl_2[/tex] (35.45g*2=70.9 grams), and this is a definite proportion.
Two natural isotopes of Chlorine are:
- Cl-35
- Cl-37
About 76% percent of Cl is found in the Cl-35 isotope, and about 24% in the Cl-37 isotope i.e. about 24% of Cl nuclei have 2 more neutrons than the average Cl nucleus.
So, if hydrogen reacts with chlorine , 76% of the Hydrogen that reacted will react with Cl-35, and the rest will react with Cl-37.
Law of definite proportions:
It states that every chemical compound contains fixed and constant proportions (by mass) of its constituent elements.
Each Hydrogen atom ends up paired to a single Chlorine atom. Moreover, the proportion of Cl-35 to Cl-37 remains constant in all samples of Chlorine that are naturally found. Thus the weight of a mol of Cl will always be 35*0.76+ 37*0.24 =35.48 or 35.45. Thus, 1 mol of hydrogen (2 grams) will always react with 1 mol of chlorine gas (35.45g*2=70.9 grams) and this proves the law of definite proportion.
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