Question

31.1 grams of O2 and 84.3 grams of F2 are placed in a container with a volume of94.9 L. Find the total pressure if the gasses are at a temperature of 55.77 ° c

Answer 1

In this question, we have:

31.1 grams of O2

84.3 grams of F2

94.9 L of total volume

55.77°C of temperature which is equal to 328.92 K

Now, to find the pressure of this container, we can find the number of moles of each gas, and add both values together making it one value of moles and then we will use the Ideal gas law to find the pressure, so let's start with O2

The molar mass of O2 is 32g/mol and we have 31.1 grams

32g = 1 mol

31.1g = x moles

x = 0.972 moles of O2

Now for F2, the molar mass is 38g/mol, and we have 84.3 grams

38g = 1 mol

84.3g = x moles

x = 2.22 moles of F2

Now we add these values, 0.972 + 2.22 = 3.192 moles

And now we can use the ideal gas law formula:

PV = nRT

Remember that R is the gas constant, 0.082

P * 94.9 L = 3.192 * 0.082 * 328.92

94.9P = 86.1

P = 0.91 atm