Question

A 0.500-mole sample of a gas has a volume of 11.2 liters at 273 k. what is the pressure of the gas? (hint: use ideal gas law equation)

Answer 1

pv =nRT

T= 273
n = 0.500
v= 11.2
R= 0.08206

p= 0.5×0.08206×273 ÷ (11.2) =10.00

Answer 2

P = 0.999375 atm

Step-by-step explanation:

To do this, we need to use the ideal gas equation which is:

PV = nRT (1)

Where:

P: Pressure (atm)

V: Volume (L)

n: moles

R: constant gas (0.082 L atm / K mol)

T: temperature (K)

From here, we can solve for P:

P = nRT/V (2)

Now, we have volume, moles, and temperature. Let's replace them in (2) to solve for P:

P = 0.5 * 0.082 * 273 / 11.2

P = 0.999375 atm

or you can round it to simply 1 atm.