Asked by Diana

What is the volume of 45.0g of nitrogen monoxide, NO, at 20 C and a pressure of 740 mm Hg?

Please someone can check my work is right or not?

NO = 14 + 16 = 30
54.0g / 30 = 33.60 L
273K/293K = 0.932 atm
740 mm Hg = 740 torr = 0.974 atm
33.60L x 0.932 x 0.974 = 30.50 L

Answer; 30.50L right or not? Than how to do? I am lost :(
Answered by Anonymous
PV=nRT

(0.974 atm)(V)=n(o.o821)(293K)

n= (45.0g)/(30.0g)=1.5 moles NO

(0.974atm)(v)=(1.5)(o.o821)(293K)

solve.
Answered by DrBob222
NO = 14 + 16 = 30
54.0g / 30 = 33.60 L <b>The problem quotes 45.0 g and not 54.0 g</b>

273K/293K = 0.932 atm <b>The Kelvin is 273 + 20 = 293 K. I don't know how you divided temperature by temperature and came out with atm.</b>

740 mm Hg = 740 torr = 0.974 atm
33.60L x 0.932 x 0.974 = 30.50 L <b>This lat line is not correct at all.</b>
Answered by DrBob222
The response by anonymous is correct.
Answered by Diana
Thank you anonymous and DrBob222!
Answered by Anonymous
no prob :)
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