Question

55. What is the density (in g/L) of hydrogen gas at 20.0 °C an pressure of 1655 psi? MISSED THIS? Read Section 6.5; Watch IWE 6.7 FLIT DOQKWWhat is

Answer 1

Solution -

First we have to convert pressure from Psi to atm by using following information -

1 atm = 14.7 psi

So,  

Pressure =

1655 psi = (1655 psi / 14.7 psi .atm^-1)

= 112 .6 atm  

This is a high pressure, we can use ideal gas equation for density determination -

PV = nRT

By rearranging,

(P/RT ) = n/V

But we know that,  

Here , n= number of moles

n = mass /molar mass

# By putting values for number of moles in ideal gas equation -

(P /RT) x molar mass = mass /V

But we know that , ( mass/Volume)= density ,so after putting this,

(P /RT) x molar mass = density

Now we can put following value into equation,

1)P=112.6 atm

2)Molar mass of hydrogen gas = 2.015 g/mol

3) R = 0.0821 L. atm. K^-1. mol^-1

4) Temperature = 20.0 ^{$\large \circ$} C

but we have to convert into' K' by = 273.15 + 20

= 293.15 K

by putting mentioned value,

density,

= (112.6 atm x 2.015 g /mol) /(0.0821 L. atm. K^-1.mol^-1 x 293.15 K)

=9.43 g/L

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