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Determine the volume of 1 $\mathrm{mol}$ of $\mathrm{CH}_{4}$ gas at 150 $\mathrm{K}$ and 1 $\mathrm{atm}$ , using Figure 9.12 .

the volume of methane gas at pressure and temperature is about.

01:08

Aadit S.

Chemistry 101

Chapter 9

Gases

University of Central Florida

Drexel University

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so continuing on with the topic of pressure. What was taking a look out here is Charles law. So at constant pressure for a given number off malls of a gas, the volume of the gas is directly proportional to the temperature in Calvin. So in a mathematical times, that is b proportional to t where V is volume, tears temperature. Or we could have, uh, the over tea is equal to K or be over. Tea is constant. We can also represented as be won over t one is equal to be to a t two. Well t one and t two are the temperature of the fast and second condition, respectively. And be one of B two of the volume of gas at the fast and second condition, respectively. So in the diagram that we've got, the graph represents a B T diagram for one mall of methane at one atmosphere pressure. So therefore, the volume of one mole of methane gas of one atmospheric pressure and 150 Calvin will be approximately 12.5 liters to 12.7 liters. So if we take a look at the graph depicting the volume and the temperature. Then we look for the intersection where the line crosses between 150 Calvin and the volume mark. So this is between 10 and 15 liters, so we add 10 and 15 liters to get 25. We then divided by two for an average of about 12.5.

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