What is the pressure in a 7.50-L flask if 0.15 mol of carbon dioxide is added to 0.33 mol of oxygen? The temperature of the mixture is 48.0$\degree$C.

Question

Quizplus · Accepted Answer

Firstly, we need to convert the temperature to Kelvin:

T = 48.0 + 273.15 = 321.15 K

Next, we can use the ideal gas law:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

We can rearrange this equation to solve for P:

P = nRT/V

We are given the volume (7.50 L), the number of moles of carbon dioxide (0.15 mol) and oxygen (0.33 mol), and the temperature (321.15 K). The gas constant R is 0.08206 L atm/mol K.

Plugging in the values:

P = (0.15 mol + 0.33 mol) * 0.08206 L atm/mol K * 321.15 K / 7.50 L

P = 1.69 atm

Therefore, the answer is choice C.

What Is the Pressure in a 7 °\degree° C A) 0

What Is the Pressure in a 7 $\degree$ C
A) 0