Calculating Density of Hydrogen Gas at 20°C & 1655psi

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The density of hydrogen gas at 20°C and 1655 psi was calculated using the formula d = P(Mm)/RT. The initial calculation converted 1655 psi to 55.31 ATM and used 293 K for temperature, resulting in a density of 4.64 g/L. However, the expected value from the textbook was 9.43 g/L, prompting a review of the pressure conversion. It was discovered that an incorrect conversion factor for inches of mercury was used instead of psi. The error was acknowledged, and the thread concluded with gratitude for the assistance received.
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Homework Statement


What is the density (g/L) of hydrogen gas at 20*c & pressure of 1655psi?


Homework Equations



d= P(Mm)/RT

Mm= molar mass

The Attempt at a Solution



I started by converting 1655 psi to 55.31 ATM. I then converted my temperature to 293 kelvins. When I plug these figures into the above equation:d= 55.31ATM(2.016g)/(.08206)(293) and I arrive at an answer of 4.64 g/L. My books gives a value of 9.43g/L which appears to be about twice as much, but I cannot figure out where I made the wrong turn. Any help would be greatly appreciated. Thanks.

Joe
 
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Recheck your psi to atm conversion.
 
Ah HA! I used the conversion factor for in Hg, not psi. Thanks a bunch, sorry for the frivolous thread.

Joe
 
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