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Chapter 11: Problem 102

In the ideal gas law, pressure must be expressed in units of _______ volume must be expressed in units of _______ temperature must be expressed in _______ and \(n\) represents the number of _______

Short Answer

Expert verified
In the Ideal Gas Law, pressure (P) must be expressed in units of atmospheres (atm), volume (V) must be expressed in units of liters (L), temperature (T) must be expressed in units of Kelvin (K), and \(n\) represents the number of moles of the gas.

Step by step solution

01

Pressure (P): Units

In the Ideal Gas Law, pressure (P) must be expressed in units of atmospheres (atm). Although there are several units to measure pressure, such as Pascal (Pa) or millimeters of mercury (mmHg), the most commonly used one in the Ideal Gas Law equation is atmospheres.
02

Volume (V): Units

In the Ideal Gas Law, volume (V) must be expressed in units of liters (L). The most common unit of volume used in this equation is liters. However, other units such as cubic meters (m^3) or milliliters (mL) might be used depending on the context, but it is important to maintain consistency in units throughout the equation.
03

Temperature (T): Units

In the Ideal Gas Law, the temperature (T) must be expressed in units of Kelvin (K). The Kelvin temperature scale starts at absolute zero (0K) and goes up from there without negative values. It is important to convert Celsius or Fahrenheit temperatures to Kelvin when using the Ideal Gas Law equation.
04

n: Representation

In the Ideal Gas Law, "n" represents the number of moles of the gas. A mole is a unit of measurement for the amount of a substance, and it is used to express quantities in terms of Avogadro's number (approximately \(6.022 \times 10^{23}\) particles).

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Most popular questions from this chapter

A student thinks he remembers reading that if you double the temperature of an ideal gas, its. pressure doubles. He is given a problem where he has an ideal gas at \(25.0{ }^{\circ} \mathrm{C}\) and \(2.5 \mathrm{~atm}\). He is asked what the temperature must be raised to in order to double the pressure to \(5.0 \mathrm{~atm}\). He answers, \(^{\prime \prime} 50.0{ }^{\circ} \mathrm{C}\), of course." Why is he wrong? What lesson should he learn about using the ideal gas law? What is the temperature increase in Celsius degrees that will double the pressure?

Carbon dioxide in a gas cylinder of unchangeable volume is at a pressure of \(25.0 \mathrm{~atm}\) at \(25^{\circ} \mathrm{C}\). When placed in the sunlight on a hot summer day, the temperature increases to \(40^{\circ} \mathrm{C}\). What is the new pressure of the \(\mathrm{CO}_{2}\) ?

A gas at \(25.0{ }^{\circ} \mathrm{C}\) occupies a volume of \(5.00\) gallons and exerts a pressure of \(755 \mathrm{~mm} \mathrm{Hg}\). Express (a) the temperature of the gas in Kelvin, (b) the volume of the gas in liters, and (c) the pressure of the gas in atmospheres.

"The older I get, the fewer hairs I have on my head." What kind of relationship (proportion or inverse proportion) exists between this gentleman's age and his hair? Explain your answer.

How many atoms of nitrogen are there in a \(230.0-\mathrm{mL}\) sample of \(\mathrm{N}_{2} \mathrm{O}_{4}\) gas that has a pressure of \(745.0 \mathrm{~mm} \mathrm{Hg}\) at \(34.0^{\circ} \mathrm{C}\) ?
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