Answer:
The Experimental Molar Volume in L/mol of the Hydrogen gas=23.36L/mol
Explanation:
We are given that
Volume of H2 at STP=52.8mL
Mass of magnesium metal ,M(Mg)=0.055g
We have to find the Experimental Molar Volume in L/mol of the Hydrogen gas.
Molar mass of Mg=24.305 g/mol
Number of moles=![\frac{given\;mass}{molar\;mass}](https://tex.z-dn.net/?f=%5Cfrac%7Bgiven%5C%3Bmass%7D%7Bmolar%5C%3Bmass%7D)
Using the formula
Number of moles of Mg=
moles
Number of moles of Mg=0.00226moles
Number of moles of Mg=Number of moles of H2
Number of moles of H2=0.00226moles
Molar volume of Hydrogen gas (H2)=![\frac{volume\;at\;STP}{No\;of\;moles\;H_2}](https://tex.z-dn.net/?f=%5Cfrac%7Bvolume%5C%3Bat%5C%3BSTP%7D%7BNo%5C%3Bof%5C%3Bmoles%5C%3BH_2%7D)
Molar volume of Hydrogen gas (H2)=![\frac{52.8}{0.00226}mL/mol](https://tex.z-dn.net/?f=%5Cfrac%7B52.8%7D%7B0.00226%7DmL%2Fmol)
Molar volume of Hydrogen gas (H2)=![\frac{52.8}{0.00226}\times 10^{-3}L/mol](https://tex.z-dn.net/?f=%5Cfrac%7B52.8%7D%7B0.00226%7D%5Ctimes%2010%5E%7B-3%7DL%2Fmol)
![1L=1000mL](https://tex.z-dn.net/?f=1L%3D1000mL)
Molar volume of Hydrogen gas (H2)=23.36L/mol
Hence, the Experimental Molar Volume in L/mol of the Hydrogen gas=23.36L/mol