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One way of purifying gaseous H2 is to pass it under high pressure through the holes of a metal's crystal structure. Palladium, which adopts a cubic closest packed structure, absorbs more H2 than any other element and is one of the metals currently used for this purpose. Although the metal-hydrogen interaction is unclear, it is estimated that the density of absorbed H2 approaches that of liquid hydrogen (70.8 g/L). What volume (in L) of gaseous H2, measured at STP, can be packed into the spaces of 1 dm3 of palladium metal

Sagot :

Okpalawalter8idn

Answer:

[tex]V=795.26L[/tex]

Explanation:

From the question we are told that:

Volume [tex]V=1dm^3=>1L[/tex]

Density [tex]\rho=70.8g/L[/tex]

Generally the equation for Density is mathematically given by

[tex]\rho =\frac{Mass}{Volume}[/tex]

Therefore

[tex]M=\rho*V[/tex]

[tex]M=70.8*1[/tex]

[tex]M=70.8g[/tex]

Since at STP

[tex]T=273K[/tex]

[tex]P=1atm[/tex]

[tex]Mass =70.8g[/tex]

Therefore

[tex]Moles\ of\ Hydrogen=\frac{Mass}{2g}[/tex]

[tex]Moles\ of\ Hydrogen=\frac{70.8}{2g}[/tex]

[tex]Moles\ of\ Hydrogen=35.4moles[/tex]

Generally the equation for Ideal gas is mathematically given by

[tex]PV=nRT[/tex]

Therefore

[tex]V=\frac{nRT}{P}[/tex]

[tex]V=\frac{35.4*0.0826*273}{1}[/tex]

[tex]V=795.3L[/tex]

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