Find the pressure in torr produced by 0.0888 mol of carbon dioxide in a 5.00 -liter vessel at 36

step 1 Hi there. This problem is working with the ideal gas equation. So that equation is PV equals NRT

Find the pressure in torr produced by 0.0888 mol of carbon...

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Key Concepts

Ideal Gas Law

The ideal gas law (PV = nRT) is a fundamental equation in chemistry and physics that relates the pressure, volume, number of moles, and temperature of an ideal gas. It provides a way to calculate any one of these variables if the others are known, and is essential for solving problems involving gases under various conditions.

Temperature Conversion

Temperature must be expressed in Kelvin when using the ideal gas law because Kelvin is the absolute temperature scale required for the proper application of the equation. Converting from Celsius to Kelvin involves adding 273.15 to the Celsius temperature.

Unit Conversion (Pressure)

In many problems, including those involving gas laws, pressure may need to be converted between different units. For example, the conversion between atmospheres and torr (or mmHg) is common, where 1 atm equals 760 torr.

Amount of Substance (Moles)

The concept of moles is fundamental to understanding the quantity of substance in a system. It quantifies the number of particles (atoms, molecules, etc.) present and is used in the ideal gas law to relate the physical state of a gas to its amount.

Transcript

00:01 Hi there.

00:02 This problem is working with the ideal gas equation.

00:06 So that equation is pv equals nrt.

00:16 And as we're reading this problem, we see that we want to solve for pressure in the unit tour.

00:25 That's what we're trying to find.

00:28 Looking at the things we are given in the problem, we are given number of moles as 0 .0888.

00:40 Moles of carbon dioxide.

00:46 We are given volume of 5 .00 liters and a temperature of 36 degrees celsius.

01:01 Now, since this is a gas law problem, we know that any temperature that we plug into any gas law equation needs to be in kelvin.

01:11 It needs to be an absolute temperature.

01:14 So i'm going to convert this to kelvin by adding 273 to it, and i get 309 kelvin.

01:24 The only thing is, we're missing now is a value for the universal gas constant, r.

01:30 Remember that is a constant.

01:32 So it is a set value, although we do have a couple of different options based upon units.

01:38 Since we want our pressure in tor, we are going to select the r that has tor as one of its units.

01:45 And that is the one that is 62 .4 liters times tor over mole kelvin.

02:00 This does have some rather units.

02:02 Unique units being that it's a constant.

02:06 In your textbook, they did go through how this was derived...

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