If two gases are present in a container, the total pressure in the container is equal to:

• A. the average of the partial pressures of both gases
• B. the product of the partial pressures of both gases
• C. the sum of the partial pressures of both gases
• D. the difference between the partial pressures of both gases

Answer: (C)

Verified step by step guidance

1. Understand Dalton's Law of Partial Pressures, which states that the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of each individual gas in the mixture.
2. Recall that the partial pressure of a gas is the pressure that gas would exert if it alone occupied the entire volume of the container at the same temperature.
3. Express the total pressure mathematically as \(P_{total} = P_1 + P_2\), where \(P_1\) and \(P_2\) are the partial pressures of the two gases.
4. Recognize that the total pressure is not the average, product, or difference of the partial pressures, but specifically their sum.
5. Conclude that the correct relationship for the total pressure in a container with two gases is the sum of their partial pressures.