Question
A container holds a mixture of two unreactive gases. The first gas in the container exerts 80.0 mmHg of pressure on the inside of the container. The total pressure inside the container is 120.0 mmHg. What is the pressure of the other gas in the container?
1.50 mmHg
150 mmHg
40.0 mmHg
200 mmHg
1.50 mmHg
150 mmHg
40.0 mmHg
200 mmHg
Answers
GPT-4o mini
To find the pressure of the other gas in the container, we can use Dalton's Law of Partial Pressures. According to this law, the total pressure in a container is equal to the sum of the partial pressures of the individual gases.
Given:
- Pressure of the first gas (P1) = 80.0 mmHg
- Total pressure (P_total) = 120.0 mmHg
We can find the pressure of the second gas (P2) using the equation:
\[ P_{total} = P_1 + P_2 \]
Rearranging the equation to solve for \( P_2 \):
\[ P_2 = P_{total} - P_1 \]
Substituting the given values:
\[ P_2 = 120.0 \, \text{mmHg} - 80.0 \, \text{mmHg} \]
\[ P_2 = 40.0 \, \text{mmHg} \]
Thus, the pressure of the other gas in the container is \( \textbf{40.0 mmHg} \).
Given:
- Pressure of the first gas (P1) = 80.0 mmHg
- Total pressure (P_total) = 120.0 mmHg
We can find the pressure of the second gas (P2) using the equation:
\[ P_{total} = P_1 + P_2 \]
Rearranging the equation to solve for \( P_2 \):
\[ P_2 = P_{total} - P_1 \]
Substituting the given values:
\[ P_2 = 120.0 \, \text{mmHg} - 80.0 \, \text{mmHg} \]
\[ P_2 = 40.0 \, \text{mmHg} \]
Thus, the pressure of the other gas in the container is \( \textbf{40.0 mmHg} \).