What is the pressure, in mm Hg, of 2.50 moles of an ideal gas if it has a volume of 50.0 liters when the temperature is 27.0° C?

84.2 mm Hg
289 mm Hg
617 mm Hg
936 mm Hg

Question

What is the pressure, in mm Hg, of 2.50 moles of an ideal gas if it has a volume of 50.0 liters when the temperature is 27.0° C?
 	
	84.2 mm Hg
	289 mm Hg
	617 mm Hg
	936 mm Hg

superhelp101 · Answer

@asib1214

somy · Answer

PV= nRT

dan815 · Answer

^noob

asib1214 · Answer

you have given three things, you can find the fourth eaisly...btw the answer is 936mm Hg

somy · Answer

P= atm - after calculation u can convert it to m Hg
V= Liter
n= mole
R= constant = 0.08206 
T= Kelvin

somy · Answer

Celsius+ 273= Kelvin

asib1214 · Answer

Given: n= 2.5 mol, V50 mol, T= 27C
Required: Pressure in mm Hg
solution: PV=nRT

before you plugin the values i suggest you should convert C into Kelvins

27 + 273 = 300K

Now rearrange the formula so that you are solving for P and it should be P=nRT/V

somy · Answer

put the values into the formula and get the answer :3

asib1214 · Answer

p= 2.5mol X 8.314(L.KPa/K.mol) X 300K divide everything by 50L

asib1214 · Answer

it shold look something like this

superhelp101 · Answer

Thank you all for all you help!!

asib1214 · Answer

|dw:1405662538096:dw|