Chemistry help! Liters, temp, pressure given?

To answer this question you use the formula PV = nRT. Where:

P = Pressure in atm

V = Volume in L

n = moles

R = 0.08206 L*atm/mol*K (gas constant)

T = temperature in K

So what you have to do here is frist change torr to atm and degrees Celsius to Kelvin.

There are 760 torr in 1 atm. So you divide:

735.5 torr * 1 atm / 760 torr = 0.97 atm

Then to change celsius to kelvin you just add 273

35.2 + 273 = 308.2K

Then you move the formula around so you are solving for n

n = PV / RT

Then you can just plug in the numbers:

n = (0.97atm)(18.86L) / (0.08206 L*atm / mol*K)(308.2K)

Everythin cancels each other out except for moles.

n = 0.723 moles

So your answer is 0.723 moles =]

Hope that helped!!!

Use the ideal gas equation: pV = nRT

p = pressure in atmospheres = 735.5 torr/760.0 torr = 0.9677 atm

V = volume in liters = 18.86 L

n = moles

R = 0.08206 L*atm/K*mol

T = 35.2 °C + 273.2 = 308.4 K

n = pV/RT = (0.9677 atm)(18.86 L)/(0.08206 L*atm/K*mol)(308.4 K) = 0.7212 mol gas in the sample

Hope this helps

Use the ideal gas law:

P V = n R T

n = P V / R T

Change units of P = 735.5 / 760 = 0.967 atm

and T = 35.2 + 273 = 308.2 K

V = 35.2 Litres

R = 0.0814

n = 0.967 x 35.2 / 0.08314 x 308.2 = 1328.39 gmoles

PV=nRT