Assuming that Nitrogen will be an ideal gas at this temperature we may use the ideal gas law:
PV=nRT
To use this law we have to have a value of R that agrees with the units that we use.
1 Torr = 1/760 atmosphere so 6680 tor = 8.789 ATM
27' C = 300.15'K
347ml = .347L
so
R= 8.314472 J/'Kmol
(8.789)(.347)/(8.314472)(300.15) = n =0.00122 moles
and of course a real man has to use scientific notation. 1.22x10-3 moles of nitrogen
19.48
8.10 L
Strange question. Volume? Perhaps density. There is no answer.
136.73 mL
all you need to do is predict what you think the answer is. this is easy
19.48
Vf = 3.0/75 (150) = 6
8.10 L
A gas occupies 40.0 L at -123 Celsius. It occupies 80 L of volume at 27 degrees Celsius.
both oxygen and nitrogen occupy space and has volume and hence are examples of matter.
468ml
If you warm it from 35 degrees Celsius to 1000 degrees Celsius, a mas will vastly increase in volume or pressure. Without knowing how you intend to allow for that, your question is unanswerable.
The volume is 0,446 L.
any increase in temperature will cause gas to occupy a larger volume, any decrease will shrink the volume to a point it becomes liquid. further decrease will cause a solid to form. at -273 degrees celsius everything is solid
Strange question. Volume? Perhaps density. There is no answer.
22412.7224278312 cm^3
A fixed quantity of gas at a constant pressure exhibits a temperature of 27 degrees Celsius and occupies a volume of 10.0 L. Use Charles's law to calculate: the temperature of the gas in degrees Celsius in atmospheres if the volume is increased to 16.0 L