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

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SUMMARY

The density of hydrogen gas at 20°C and a pressure of 1655 psi is calculated using the formula d = P(Mm)/RT. The correct conversion of 1655 psi to atmospheres is 55.31 ATM, and the temperature is converted to 293 K. The molar mass (Mm) of hydrogen is 2.016 g/mol, leading to a calculated density of 4.64 g/L. The discrepancy with the book's value of 9.43 g/L was due to an incorrect conversion factor used for pressure.

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  • Understanding of the Ideal Gas Law
  • Knowledge of unit conversions (psi to ATM)
  • Familiarity with molar mass calculations
  • Basic algebra for solving equations
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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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