Question

Calculate the Experimental Molar Volume in L/mol of the Hydrogen gas, H2, if the volume of H2 at STP is 52.8 mL and the mass of Magnesium metal, Mg, used in the experiment is 0.055 g.

Answer 1

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=$\frac{given\;mass}{molar\;mass}$

Using the formula

Number of moles of Mg=$\frac{0.055}{24.305}$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)=$\frac{volume\;at\;STP}{No\;of\;moles\;H_2}$

Molar volume of Hydrogen gas (H2)=$\frac{52.8}{0.00226}mL/mol$

Molar volume of Hydrogen gas (H2)=$\frac{52.8}{0.00226}\times 10^{-3}L/mol$

$1L=1000mL$

Molar volume of Hydrogen gas (H2)=23.36L/mol

Hence, the Experimental Molar Volume in L/mol of the Hydrogen gas=23.36L/mol