What is the pressure (in torr) inside a 2.0 liter flask at 26°C and 27.2 grams of oxygen gas?

Question

1.59 x 104 torr = 20.9 atm = 2.11 x 103 kPa
793 torr = 1.04 atm = 106 kPa
7.93 x 103 torr = 10.4 atm = 1.06 x 103 kPa
2.54 x 105 torr = 334 atm = 3.39 x 104 kPa

Answer 1

Whenever you have to solve for the pressure, you use the
PV=nRT equation, where
P = pressure
V = volume (in liters)
n = number of moles
R = .016 (in torrs)
T = temperature (in Kelvin).

Here, you want to solve for P - for the pressure. So first you need to find what n is, what T is, and then you just plug in.

number of moles = (grams)/(atomic mass). You have 27.2 grams of Oxygen, and its atomic mass is 32.
27.2/32 = .85
So you have 0.85 moles of Oxygen.

Now you need to solve for T. Temperature in Kelvin is 273 degrees more than C.
26°C + 273 = 299°K .

Now, you have all the information you need to plug in for the equation
PV = nRT.
P * 2.0 = .85 * .016 * 299
or
P = (.85 * .016 * 299) / 2.0
P = 2.0332 atm = 1,545.232 torr

Answer 2

you would be able to desire to discover the moles of O2, mandatory for the reaction VO2 = nO2*R*T/P (nO2 = no of moles O2) Use stochiometry to get moles of O2: 5O2 + C3H8 ----> 3CO2 + 4H20 The no moles of O2 is 5 cases the no of moles of C3H8. discover the no of moles of C3H8 from the gasoline regulation nPr = P*VPr/R*T nO2 = 5*nPr = 5*P*VPr/R*T V = 5*P*VPr/R*T * R*T/P = 5*VPr = 15.0 L In different words, if the temperature and stress are an identical, the quantity ratio is an identical because of fact the mole ratio,

Answer 3

i agree with the previous user except one thing
R = 22.4/273
because of that R=0.082 approximately
the other ones correct :)

Answer 4

One will be bigger than the other.