Chapter 8: Q. 8.56 (page 278)

In a gas mixture, the partial pressure are argon $415 m m H g$ , neon $75 m m H g$ , and nitrogen $125 m m H g$ . What is the total pressure, in $m m H g$ , exerted by the gas mixture?

Short Answer

Expert verified

The total pressure is $615 m m H g$ .

Step by step solution

Given Information

We need to find the total pressure.

Simplify

In a gas, mixture, each gas exerts its partial pressure, which is the pressure it would exert if it were the gas in the container. Dalton's law that the total pressure of a gas mixture is the sum of the partial pressures of the gases in the mixture.

The total pressure is:

Argon is $P_{A r} = 415 m m H g$

Neon is $P_{n e} = 75 m m H g$

Nitrogen is $P_{n} = 125 m m H g$

$P_{t o t a l} = P_{A r} + P_{n e} + P_{n} = 415 m m H g + 75 m m H g + 125 m m H g = 615 m m H g$

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In a gas mixture, the partial pressure are argon $415 m m H g$ , neon $75 m m H g$ , and nitrogen $125 m m H g$ . What is the total pressure, in $m m H g$ , exerted by the gas mixture?

Short Answer

Step by step solution

Given Information

Simplify

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In a gas mixture, the partial pressure are argon 415mmHg, neon 75mmHg, and nitrogen 125mmHg. What is the total pressure, in mmHg, exerted by the gas mixture?

Short Answer

Step by step solution

Given Information

Simplify

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Inorganic Chemistry

Chemical Reactions

The Earths Atmosphere

Organic Chemistry

Nuclear Chemistry

Study anywhere. Anytime. Across all devices.

In a gas mixture, the partial pressure are argon $415 m m H g$ , neon $75 m m H g$ , and nitrogen $125 m m H g$ . What is the total pressure, in $m m H g$ , exerted by the gas mixture?