could u guys tell if im right with these:(adsbygoogle = window.adsbygoogle || []).push({});

1)

a) calculate the volume occupied by 6.5 g of Nitrogen gas @ STP

[tex]\frac{1_{mol}}{28g_{N_2}}=\frac{x_{mol}}{6.5g}[/tex]

[tex]x\sim0.23[/tex]

[tex]\frac{101.3*V}{273*0.23}=8.31[/tex]

so i got that 6.5 grams of N_2 is ~ 0.23 mol so using the ideal gas law i solved for V getting5.15 L

b) calculate the volume occupied by this mass of gas at -40.0 C and 65.0 kPa

[tex]\frac{65*V}{233*0.23}=8.31[/tex]

so i did the same thing as "a" except filled in those values of temperature(kelvin) and pressure, i got6.9 L

2)

this one im not so sure about:

what is the molar mass of a gas if 375 cm^3 have mass 0.800 g at 85 C and 100.7 kPa?

using the ideal gas law i did:

[tex]\frac{100.7*0.375}{358*n}=8.31[/tex]

[tex]n\sim ~ 0.013 mol[/tex]

then i divided 0.800g by 0.013 mol and got ~61.5grams molar mass

is that right?

thanks in advance

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# Homework Help: Gas laws corrections

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