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Chapter 10: Problem 95

What is meant by the partial pressure of a gas?

Short Answer

Expert verified
Define partial pressure and explain its importance in a mixture of gases, particularly in biological systems like gas exchange during respiration.

Step by step solution

01

Define Partial Pressure

Partial pressure of a gas is the pressure that a gas in a mixture would exert if it alone occupied the same volume at the same temperature. In other words, it is the pressure that each gas contributes to the total pressure of the mixture.
02

Dalton's Law of Partial Pressures

To better understand the concept of partial pressure, we need to discuss Dalton's Law of Partial Pressures. This law 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. Mathematically, it can be represented as follows: \[P_{total} = P_1 + P_2 + P_3 + ... + P_n\] Where \(P_{total}\) is the total pressure of the mixture and \(P_1, P_2, P_3, ...\), are the partial pressures of each individual gas in the mixture.
03

Importance of Partial Pressure in Gas Exchange

Partial pressure of gases plays a key role in biological systems' gas exchange processes, such as respiration. In the human respiratory system, the partial pressure is the driving force for the movement of oxygen and carbon dioxide between the lungs and blood cells. A higher partial pressure of oxygen in the lungs compared to the blood drives oxygen to move into the blood. Conversely, a higher partial pressure of carbon dioxide in the blood drives it to move into the lungs, where it can be exhaled. In summary, the partial pressure of a gas is the pressure it contributes to the total pressure of a mixture of gases. It is important for various applications, including gas exchange processes in biological systems.

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Most popular questions from this chapter

The volume of a quantity of gas at 1.00 atm is compressed from \(3.25 \mathrm{L}\) to \(2.24 \mathrm{L} .\) What is the final pressure of the gas if there is no change in temperature?

The volume of a weather balloon is \(200.0 \mathrm{L}\) and its internal pressure is 1.17 atm when it is launched at \(20^{\circ} \mathrm{C}\). The balloon rises to an altitude in the stratosphere where its internal pressure is \(63 \mathrm{mmHg}\) and the temperature is \(210 \mathrm{K} .\) What is the volume of the balloon at this altitude?

Rank the gases \(\mathrm{NO}, \mathrm{NO}_{2}, \mathrm{N}_{2} \mathrm{O}_{4},\) and \(\mathrm{N}_{2} \mathrm{O}_{5}\) in order of increasing root-mean-square speed at \(0^{\circ} \mathrm{C}\).

The reaction between potassium super-oxide and carbon dioxide is used to produce \(0.200 \mathrm{L}\) of \(\mathrm{O}_{2},\) which is collected over water at \(25.0^{\circ} \mathrm{C} .\) The atmospheric pressure is 750.0 torr. The vapor pressure of water at \(25.0^{\circ} \mathrm{C}\) is 24.0 torr. How many moles of \(\mathrm{O}_{2}\) have becn collected? $$4 \mathrm{KO}_{2}(s)+2 \mathrm{CO}_{2}(g) \rightarrow 2 \mathrm{K}_{2} \mathrm{CO}_{3}(s)+3 \mathrm{O}_{2}(g)$$

Miners' Lamps Before the development of reliable batterics, miners' lamps burned acetylene produced by the reaction of calcium carbide with water: $$\mathrm{CaC}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{C}_{2} \mathrm{H}_{2}(g)+\mathrm{CaO}(s)$$ Suppose a lamp uses \(4.8 \mathrm{L}\) of acetylene per hour at 1.02 atm pressure and \(25^{\circ} \mathrm{C}\) a. How many moles of \(\mathrm{C}_{2} \mathrm{H}_{2}\) are used per hour? b. How many grams of calcium carbide are consumed for a four-hour shift?
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