Question

1. what is the total pressure of a gas mixture containing partial pressures of 0.23 atm, 0.42 atm, and 0.89 atm?

a. 0.18 atm
b. 0.51 atm
c. 1.54 atm
d. 0.42 atm

Explanation:

Step1: Recall Dalton's Law of Partial Pressures

Dalton's Law states that the total pressure \(P_{total}\) of a gas mixture is the sum of the partial pressures \(P_i\) of each component gas. Mathematically, \(P_{total}=\sum_{i = 1}^{n}P_i\).

Step2: Substitute the given partial pressures

Here, \(P_1 = 0.23\ \text{atm}\), \(P_2=0.42\ \text{atm}\), and \(P_3 = 0.89\ \text{atm}\). Then \(P_{total}=0.23 + 0.42+0.89\).

Step3: Perform the addition

First, \(0.23+0.42 = 0.65\), then \(0.65 + 0.89=1.54\).

Answer:

C. \(1.54\ \text{atm}\)