Chemistry review

Question

How many moles of air are in a 0.125L flask of the pressure is 1.0 atm and the temperature is 273K

Answer 1

We will use the ideal gas law:

R = PV/nT

where R = 0.0821 L*atm/K*mol, P = pressure (atm), V = Volume(Liter), n = number of moles, and T = temperature(Kelvin)

We will rearrange the equation to solve for n:

n = PV/RT = (1.0 atm* 0.125 L) / 0.0821 L*atm/K*mol * 273 = 5.57 x 10^-3 mol.

There will be 5.57 x 10^-3 moles.

Answer 2

Use the ideal gas law equation.

PV = nRT

P = 1.0 atm

V = 0.125 L

n = ?

R = 0.0821 L atm mol^-1 K^-1

T = 273 K

Rearrange and solve for n, which is the # of moles.

n = PV / RT

= (1.0 atm x 0.125 L) / (0.0821 L atm mol^-1 K^-1 x 273 K)

= 0.0056 moles