Question

A 519.93 gram sample of N2O is in a 7.05 L container. What is the pressure of the gas in atmospheres when the temperature is 125.63K?

Answer 1

Answer:

17.27 atm

Explanation:

Use the ideal gas law or PV = nRT

We are solving for pressure here so lets isolate for P before we plug in values:

$P = \frac{nRT}{V}$

So first to get n or the number of moles we need to convert the grams of N2O to moles of N2O. We can do this by multiplying by the inverse of the molar mass like so:

$\frac{519.93g(N2O)}{1} \frac{mol}{44.013g(N2O)}$

Our grams of N2O would cancel and give us 11.813 mol of N2O

Now all thats left is to plug in and solve with the correct value for R which in this case for all of our units to cancel is 0.08206

$P = \frac{(11.813)(0.08206)(125.63)}{7.05}$

P = 17.27 atm

(I would double check the calculator work if it is for correctness just be sure)

Answer 2

Answer:

The pressure of the gas is 17.27 atm

Explanation:

Step 1: Data given

Mass of N2O = 519.93 grams

Molar mass of N2O = 44.01 g/mol

Volume = 7.05 L

Temperature = 125.63 K

Step 2: Calculate moles N2O

Moles N2O = mass N2O / molar mass N2O

Moles N2O = 519.93 grams / 44.01 g/mol

Moles N2O = 11.81 moles

Step 3: Calculate pressure

p*V = n*R*T

p = (n*R*T)/V

⇒with p = the pressure of the gas = TO BE DETERMINED

⇒with n = the number of moles of gas = 11.81 moles

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 125.63 K

⇒with V  = the volume = 7.05 L

p = (11.81 * 0.08206 * 125.63) / 7.05

p = 17.27 atm

The pressure of the gas is 17.27 atm