471.45g of Mg3P2
Here’s the answer and work shown
Answer:
, The partial pressure of O2 is = 21 atm
Explanation:
The concept is the pressure exerted by each gas is independent of one another or in other words independent of the pressure exerted by all other gases present.
This means that total pressure is the sum of the individual pressure of each gas by dalton's law.
![P_{Total}= P_O_2+P_{Ar}+P_{He}](https://tex.z-dn.net/?f=P_%7BTotal%7D%3D%20P_O_2%2BP_%7BAr%7D%2BP_%7BHe%7D)
So, putting the given values we get
43 = P_O2 +15+7
P_O2 = 21 atm
Therefore, The partial pressure of O2 is = 21 atm
Answer:
Yea.....where is the article and the 6 questions?
Answer:
The answer is "
".
Explanation:
Please find the complete question in the attached file.
Total Moles of
= moles of
![= \frac{mass}{molar \ mass \ of MgSO_4}\\\\= \frac{0.450}{120.37}\\\\ = 0.0037385 \ mol](https://tex.z-dn.net/?f=%3D%20%5Cfrac%7Bmass%7D%7Bmolar%20%5C%20mass%20%5C%20of%20MgSO_4%7D%5C%5C%5C%5C%3D%20%5Cfrac%7B0.450%7D%7B120.37%7D%5C%5C%5C%5C%20%3D%200.0037385%20%5C%20mol)
![Mg_2^{+} + EDTA4^{-} \longrightarrow Mg(EDTA)2^{-}](https://tex.z-dn.net/?f=Mg_2%5E%7B%2B%7D%20%2B%20EDTA4%5E%7B-%7D%20%5Clongrightarrow%20%20Mg%28EDTA%292%5E%7B-%7D)
EDTA mol in 37.6 mL of solution = 50.0 mL of ![Mg2^{+}](https://tex.z-dn.net/?f=Mg2%5E%7B%2B%7D)
total moles of ![Mg2^{+}](https://tex.z-dn.net/?f=Mg2%5E%7B%2B%7D)
![= \frac{50.0}{500} \times 0.0037385\\\\= 3.7385 \times 10^{(-4)} \ mol\\](https://tex.z-dn.net/?f=%3D%20%5Cfrac%7B50.0%7D%7B500%7D%20%5Ctimes%20%200.0037385%5C%5C%5C%5C%3D%203.7385%20%5Ctimes%20%2010%5E%7B%28-4%29%7D%20%5C%20%20mol%5C%5C)
![Ca2^{+} + EDTA4^{-} \longrightarrow Ca(EDTA)2^{-}](https://tex.z-dn.net/?f=Ca2%5E%7B%2B%7D%20%2B%20EDTA4%5E%7B-%7D%20%5Clongrightarrow%20Ca%28EDTA%292%5E%7B-%7D)
EDTA moles in a solution of 1.40 mL
the solution of EDTA moles.
![= \frac{1.40}{37.6} \times 3.7385 \times 10^{(-4)} \\\\= 1.392 \times 10^{(-5)}\ mol\\\\](https://tex.z-dn.net/?f=%3D%20%5Cfrac%7B1.40%7D%7B37.6%7D%20%5Ctimes%20%203.7385%20%5Ctimes%20%2010%5E%7B%28-4%29%7D%20%5C%5C%5C%5C%3D%201.392%20%5Ctimes%20%2010%5E%7B%28-5%29%7D%5C%20%20mol%5C%5C%5C%5C)
Mass of
mole
the molar mass of
![= 1.392 \times 10^{(-5)} \times 100.09\\\\= 0.00139 \ g\\\\ = 1.39 \ mg](https://tex.z-dn.net/?f=%3D%201.392%20%5Ctimes%2010%5E%7B%28-5%29%7D%20%5Ctimes%20100.09%5C%5C%5C%5C%3D%200.00139%20%5C%20g%5C%5C%5C%5C%20%3D%201.39%20%5C%20mg)