A 1.00 leader flask can withstand a pressure 5.00 ATM without busting can the classical 5.00 g of 02 at a temperature 25°

Answer 1

To determine if the classical 5.00 g of O2 at a temperature of 25°C can withstand a pressure of 5.00 ATM in a 1.00 L flask, we need to use the ideal gas law equation:

PV = nRT

Where:
P = pressure (in ATM)
V = volume (in L)
n = number of moles of gas
R = ideal gas constant (0.0821 L*ATM/mol*K)
T = temperature (in Kelvin)

First, let's convert the mass of O2 into moles:
1 mol of O2 = 32 g
5.00 g of O2 = 5.00 g / 32 g/mol ≈ 0.15625 mol

Next, convert the temperature from Celsius to Kelvin:
25°C + 273 = 298 K

Now, we can plug the values into the ideal gas law equation:
(5.00 ATM)(1.00 L) = (0.15625 mol)(0.0821 L*ATM/mol*K)(298 K)

5.00 = (0.15625)(0.0821)(298)
5.00 = 3.66961

Since the calculated pressure is less than the given pressure of 5.00 ATM, the classical 5.00 g of O2 at a temperature of 25°C in a 1.00 L flask can withstand the pressure of 5.00 ATM without busting.