Question

The pattern of O2 in a 1.00 L container at 20C is 0.370 atm. what will the pressure inside the container be 0.01000mol CO2 is added to it?

A. 0.611 atm
B. 0.380 atm
C. 1.01 atm
D. 0.241 atm

Answer 1

To find the final pressure inside the container after adding CO2, we use the ideal gas law equation PV = nRT. The initial number of moles of O2 can be found using the equation n = PV / RT. After adding the moles of CO2, the total number of moles is calculated. The final pressure is then found using the ideal gas law equation P = nRT / V.

Step-by-step explanation:

To find the final pressure inside the container after adding 0.01000 mol CO2, we need to consider the ideal gas law. The ideal gas law equation is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature.

First, we need to find the initial number of moles of O2. Given that the initial pressure is 0.370 atm, we can rearrange the ideal gas law equation to find the initial number of moles:

n = PV / RT = (0.370 atm)(1.00 L) / (0.0821 L·atm/mol·K)(293 K) = 0.0152 mol

After adding 0.01000 mol CO2, the total number of moles is 0.0152 mol + 0.01000 mol = 0.0252 mol.

Using the same ideal gas law equation, we can now find the final pressure:

P = nRT / V = (0.0252 mol)(0.0821 L·atm/mol·K)(293 K) / 1.00 L = 0.611 atm.