Visible light is the wave and it has 10^-6
Answer:
The the empirical formula for magnesium chloride based on this experiment will be ![MgCl_{2}](https://tex.z-dn.net/?f=MgCl_%7B2%7D)
Explanation:
Given that,
Mass of Mg = 0.50 g
Mass of magnesium chloride found = 1.99 g
Let the formula of magnesium chloride be ![Mg_{x}Cl_{y}](https://tex.z-dn.net/?f=Mg_%7Bx%7DCl_%7By%7D)
We know that,
Molar mass of Mg= 24 g/mol
Molar mass of magnesium chloride = (24x+35.5y) g/mol
We need to calculate the moles of Mg
Using formula of moles
![Number\ of\ moles=\dfrac{mass}{molar\ mass\ of\ Mg}](https://tex.z-dn.net/?f=Number%5C%20of%5C%20moles%3D%5Cdfrac%7Bmass%7D%7Bmolar%5C%20mass%5C%20of%5C%20Mg%7D)
Put the value into the formula
![Number\ of\ moles=\dfrac{0.50}{24}](https://tex.z-dn.net/?f=Number%5C%20of%5C%20moles%3D%5Cdfrac%7B0.50%7D%7B24%7D)
![Number\ of\ moles=0.020\ mole](https://tex.z-dn.net/?f=Number%5C%20of%5C%20moles%3D0.020%5C%20mole)
We need to calculate the mole of magnesium chloride
Using formula of moles
![Number\ of\ moles=\dfrac{mass}{molar\ mass\ of\ magnesium\ chloride}](https://tex.z-dn.net/?f=Number%5C%20of%5C%20moles%3D%5Cdfrac%7Bmass%7D%7Bmolar%5C%20mass%5C%20of%5C%20magnesium%5C%20chloride%7D)
Put the value into the formula
![Number\ of\ moles=\dfrac{1.99}{24x+35.5y}\ mole](https://tex.z-dn.net/?f=Number%5C%20of%5C%20moles%3D%5Cdfrac%7B1.99%7D%7B24x%2B35.5y%7D%5C%20mole)
The reaction will be,
![Mg+HCl\Rightarrow Mg_{x}Cl_{y}+H_{2}](https://tex.z-dn.net/?f=Mg%2BHCl%5CRightarrow%20Mg_%7Bx%7DCl_%7By%7D%2BH_%7B2%7D)
We need to calculate the value of x and y
Using number of moles of Mg in reactant and product
Moles of Mg atom in reactant=Moles of Mg atom in product
![\dfrac{0.50}{24}=x\times\dfrac{1.99}{24x+35.5y}](https://tex.z-dn.net/?f=%5Cdfrac%7B0.50%7D%7B24%7D%3Dx%5Ctimes%5Cdfrac%7B1.99%7D%7B24x%2B35.5y%7D)
![0.020(24x+35.5y)=x\times1.99](https://tex.z-dn.net/?f=0.020%2824x%2B35.5y%29%3Dx%5Ctimes1.99)
![0.48x+0.71y=1.99x](https://tex.z-dn.net/?f=0.48x%2B0.71y%3D1.99x)
![0.71y=(1.99-0.48)x](https://tex.z-dn.net/?f=0.71y%3D%281.99-0.48%29x)
![\dfrac{x}{y}=\dfrac{0.71}{1.99-0.48}](https://tex.z-dn.net/?f=%5Cdfrac%7Bx%7D%7By%7D%3D%5Cdfrac%7B0.71%7D%7B1.99-0.48%7D)
![\dfrac{x}{y}=0.47\approx0.5](https://tex.z-dn.net/?f=%5Cdfrac%7Bx%7D%7By%7D%3D0.47%5Capprox0.5)
![\dfrac{x}{y}=\dfrac{1}{2}](https://tex.z-dn.net/?f=%5Cdfrac%7Bx%7D%7By%7D%3D%5Cdfrac%7B1%7D%7B2%7D)
Hence, The the empirical formula for magnesium chloride based on this experiment will be ![MgCl_{2}](https://tex.z-dn.net/?f=MgCl_%7B2%7D)
Answer: Blue liquid density = 45 grams/70 mL Density = .64 g/mL Yellow liquid density = 80 grams/ 65mL Density = 1.23 g/mL After the liquids are combined the blue less dense liquid will rise to the top, while the yellow more dense liquid will sinks to the bottom.