Question

a flask contains argon, helium, and fluorine gases. the partial pressures of each are 14.1 torr, 12.2 torr, and 8.6 torr, respectively. what is the total pressure in the flask in torr?

Explanation:

Step1: Recall Dalton's Law of Partial Pressures

Dalton's Law states that the total pressure \( P_{total} \) of a mixture of gases is the sum of the partial pressures of the individual gases. So, \( P_{total} = P_1 + P_2 + P_3 \), where \( P_1 \), \( P_2 \), and \( P_3 \) are the partial pressures of argon, helium, and fluorine respectively.

Step2: Identify the partial pressures

The partial pressures are \( P_{argon} = 14.1 \) Torr, \( P_{helium} = 12.2 \) Torr, and \( P_{fluorine} = 8.6 \) Torr.

Step3: Calculate the total pressure

Substitute the values into the formula: \( P_{total} = 14.1 + 12.2 + 8.6 \). First, add 14.1 and 12.2: \( 14.1 + 12.2 = 26.3 \). Then add 8.6 to the result: \( 26.3 + 8.6 = 34.9 \).

Answer:

34.9