A mixture of nitrogen (N₂) and helium has a volume of 250 mL at 30 °C and a total pressure of 745 mmHg. (8.5, 8.6, 8.7)a. If the partial pressure of helium is 32 mmHg, what is the partial pressure of the nitrogen?

Verified step by step guidance

1. Identify the given values: total pressure (P_total) = 745 mmHg and partial pressure of helium (P_He) = 32 mmHg.
2. Recall Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is the sum of the partial pressures of each individual gas: P_total = P_N2 + P_He.
3. Rearrange the equation to solve for the partial pressure of nitrogen (P_N2): P_N2 = P_total - P_He.
4. Substitute the known values into the equation: P_N2 = 745 mmHg - 32 mmHg.
5. Calculate the partial pressure of nitrogen using the values from the previous step.

Key Concepts

Dalton's Law of Partial Pressures

Dalton's Law states that in a mixture of gases, the total pressure exerted is equal to the sum of the partial pressures of each individual gas. This principle allows us to calculate the pressure of one gas in a mixture if we know the total pressure and the partial pressures of the other gases present.

Partial Pressure

Partial pressure refers to the pressure that a single gas in a mixture would exert if it occupied the entire volume alone at the same temperature. It is a crucial concept for understanding gas behavior in mixtures and is calculated using the formula: P_total = P_helium + P_nitrogen.

Gas Laws

Gas laws describe the relationships between pressure, volume, temperature, and the number of moles of a gas. In this context, understanding how these variables interact helps in solving for unknown pressures and volumes in gas mixtures, particularly under varying conditions.