Question

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

Answer 1

`V=795.26L`

Step-by-step explanation:

From the question we are told that:

Volume
`V=1dm^3=>1L`

Density
`\rho=70.8g/L`

Generally the equation for Density is mathematically given by

`\rho =(Mass)/(Volume)`

Therefore

`M=\rho*V`

`M=70.8*1`

`M=70.8g`

Since at STP

`T=273K`

`P=1atm`

`Mass =70.8g`

Therefore

`Moles\ of\ Hydrogen=(Mass)/(2g)`

`Moles\ of\ Hydrogen=(70.8)/(2g)`

`Moles\ of\ Hydrogen=35.4moles`

Generally the equation for Ideal gas is mathematically given by

`PV=nRT`

Therefore

`V=(nRT)/(P)`

`V=(35.4*0.0826*273)/(1)`

`V=795.3L`