A 8.75-L container holds a mixture of two gases at 23 °C. The partial pressures of gas A and gas B, respectively, are 0.317 atm and 0.755 atm. If 0.100 mol of a third gas is added with no change in volume or temperature, what will the total pressure become?
p of gas C = nRT/V. Substitute and solve for pressure of gas C.
Then Ptotal = pA + pB + pC = about 1.35 atm.
To find the total pressure after adding the third gas, we need to use the concept of Dalton's Law of partial pressures. According to Dalton's Law, the total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas.
First, let's find the initial total pressure of the mixture. We add the partial pressures of gas A and gas B:
Initial total pressure = Partial pressure of gas A + Partial pressure of gas B
Initial total pressure = 0.317 atm + 0.755 atm
Initial total pressure = 1.072 atm
Now, since the volume and temperature remain constant, we can directly apply Dalton's Law to find the new total pressure after adding the third gas.
The partial pressure of the third gas will be the same as the partial pressure of gas A, which is 0.317 atm. Therefore, the new total pressure will be:
New total pressure = Initial total pressure + Partial pressure of the third gas
New total pressure = 1.072 atm + 0.317 atm
New total pressure = 1.389 atm
Therefore, the total pressure will become 1.389 atm after adding the third gas to the mixture.