When 0.215 mol of a gas is placed into a 34.25 mL container at 125.0°C, 1 it will exert a pressure on the container. Justin has been asked to
calculate the pressure that this gas will exert on the container in kPa, then
to
go into the lab and measure this pressure. What will he determine is the
pressure of the gas?

205.12 atm

Explanation:

Using the ideal gas law equation:

PV = nRT

Where;

P = pressure (atm)

V = volume (L)

R = 0.0821 Latm/perK)

T = temperature (K)

n = number of moles (mol)

According to the information in this question;

P = ?

V = 34.25 mL = 34.25 ÷ 1000 = 0.03425L

n = 0.215 mol

T = 125.0°C = 125 + 273 = 398K

Using PV = nRT

P = nRT ÷ V

P = (0.215 × 0.0821 × 398) ÷ (0.03425)

P = 7.025 ÷ 0.03425

P = 205.12 atm

sure what is it? ^w^

did anyone actually do this? like if anyone has submitted this i rly need .