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makayyafreeman
10.06.2021 •
Chemistry
When the nuclide polonium-218 undergoes alpha decay:
a. The name of the product nuclide is .
b. The symbol for the product nuclide is .
Write a balanced nuclear equation for the following: The nuclide polonium-218 undergoes alpha emission.
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Ответ:
a): The name of the product nuclide is lead-214
b): The symbol of the product nuclide is Pb-218
Explanation:
There are three types of decay processes:
Alpha decayBeta decayGamma decayAlpha decay is the decay process that happens when a heavy nucleus decays into a light nucleus with the release of an alpha particle. This alpha particle carries a charge of +2 units and has a mass of 4 units. It is also known as the helium nucleus. The general equation for this decay process is:
The nuclear equation for the alpha decay of Po-218 follows:
Hence, the name of the product nuclide is lead-214 and the symbol is Pb-218.
Ответ:
a.3.2204 g
b.Ag+ = 0 M
NO3? = 0.105 M
Ca2+ = 0.07M
Cl? =0.035 M
Explanation:
The balanced equation for this reaction is:
mol of![AgNO_{3}](/tpl/images/0320/7487/9725a.png)
mol of![CaCl_{2}](/tpl/images/0320/7487/a0038.png)
from the reaction stoichiometry we know that we need 2 moles of
per every mol of
.
so for 0.01498 mol of
we need 0.01498*2 =0.02996 mol of
. Since we have just 0.02247 mol, this will be the reaction limit reagent for this reaction.
we will use all the![AgNO_{3}](/tpl/images/0320/7487/9725a.png)
mol of
used =![\frac{0.02247}{2}=0.011235mol](/tpl/images/0320/7487/606f7.png)
For the calculation we always use the limit reagent.
a. How many grams of silver chloride.
From the reaction stoichiometry we know that 2 mol of
produce 2 mol of AgCl so, 0.02247 mol of
will the same number of mol of AgCl.
AgCl produced = 0.02247 mol
molecular weight of AgCl = 143.32 g/mol
mass of AgCl =![mol*Mw = 0.02247 mol*143.32 \frac{g}{mol}=3.2204 g](/tpl/images/0320/7487/97b86.png)
b.concentrations of each ion
volume of the remained solution 107 mL + 107mL= 214 mL or 0.214 L
concentration =![\frac{0.02247 mol}{0.214L}=0.105 M](/tpl/images/0320/7487/6fa53.png)
following the same analysis for made for
we know that
did not precipitated so we have the same number of moles of
in the original sample but in a different volume
concentration =![\frac{0.01498 mol}{0.214L}=0.07 M](/tpl/images/0320/7487/42ffe.png)
the Cl in the solution after the precipitation will be the Cl that did not reacted since all the Cl that reacted to produce AgCl precipitated.
Cl that reacted is the same number of AgCl produced this is=0.02247 mol
Cl before the reaction is 2 times the number of moles of
in the sample this is: 0.01498*2 =0.02996 mol
Cl remained = 0.02996 mol -0.02247 mol=0.00749 mol
concentration =![\frac{0.00749 mol}{0.214L}=0.035 M](/tpl/images/0320/7487/be15d.png)