Please round off the final answer in two decimal places. Answer only the numerical value and don't include the units. 
Prepare papers and pen The vapor pressure of Gas A (MW=98) is 17.6 psig. The vapor pressure of Gas B (MW=112) is 95.6 psig. It was used to prepare a 500 mL of 1:4 gas combination of gas A and gas B respectively. 

What is the partial pressure of gas A in the mixture?

To find the partial pressure of gas A in the mixture, we use the formula for partial pressure in a gas mixture:

\[
P_A = \left( \frac{n_A}{n_A + n_B} \right) \times P_{\text{total}}
\]

1. Since it’s a 1:4 mixture, the ratio of gas A to gas B is 1 part gas A to 4 parts gas B. Thus, for every 5 parts of the total, 1 part is gas A.

2. Calculate the total pressure of the mixture using Dalton's Law of Partial Pressures, which sums the individual pressures of the gases. Here, \( P_{\text{total}} = 17.6 + 95.6 = 113.2 \) psig.

3. The fraction of gas A in the mixture is \( \frac{1}{5} \).

4. Thus, the partial pressure of gas A is:

\[
P_A = \frac{1}{5} \times 113.2 = 22.64
\]

The rounded-off final answer is:

**22.64**

Please round off the final answer in two decimal places. Answer only the numerical value and don't include the units. Prepare papers and pen The vapor pressure of Gas A (MW=98) is 17.6 psig. The vapor pressure of Gas B (MW=112) is 95.6 psig. It was used to prepare a 500 mL of 1:4 gas combination of gas A and gas B respectively. What is the partial pressure of gas A in the mixture?

Learn how to find the partial pressure of Gas A in a mixture with Gas B using Dalton's Law of Partial Pressures. Given: Gas A vapor pressure = 17.6 psig, Gas B vapor pressure = 95.6 psig, with a 1:4 gas mixture ratio. Solution includes calculating the total pressure and applying the formula for partial pressure.

Math Problem Statement

Solution

Ask a new question for Free

By Image

Math Problem Analysis

Mathematical Concepts

Formulas

Theorems

Suitable Grade Level

Related Recommendation