The pressure exerted by 6.04 mol of nitrogen monoxide at a temperature of 18^∘ C is 17.2 atm. Wh

The pressure exerted by 6.04 mol of nitrogen monoxide at a...

Key Concepts

Ideal Gas Law

The Ideal Gas Law is a fundamental equation in chemistry and physics that relates the pressure (P), volume (V), number of moles (n), and temperature (T) of an ideal gas through the equation PV = nRT. This law provides a method to calculate any one of these properties if the others are known, making it a crucial tool for understanding the behavior of gases under various conditions.

Gas Constant

The gas constant, commonly represented by R, is a proportionality factor in the Ideal Gas Law that connects the measurable quantities of pressure, volume, and temperature of a gas. Its value depends on the units used in the equation and is essential for ensuring that the calculation is dimensionally consistent, allowing for correct conversion and computation of gas properties.

Temperature Conversion

Temperature conversion, particularly converting degrees Celsius to Kelvin, is a necessary step when using the Ideal Gas Law because the temperature must be expressed in an absolute scale. The conversion is done by adding 273.15 to the Celsius reading, ensuring that the temperature variable correctly reflects thermodynamic principles used in gas calculations.

Transcript

00:01 Hi there.

00:03 For this problem, we are going to be using the ideal gas equation, which is pv equals nrt.

00:13 And as we read through the problem, we see that we would like to solve for volume.

00:20 So that is my unknown in this problem.

00:23 Volume is going to be in liters.

00:27 Looking at the information that we do know in this problem, we know number of moles.

00:32 Number of moles is 6 .04.

00:39 Moles of no, nitrogen monoxide.

00:42 We have a temperature that is given of 18 degrees celsius.

00:52 Since this is a gas law problem, all gas law problems need absolute temperature, or in other words, temperature in kelvin.

01:01 So i'm going to go ahead and convert this to kelvin, and i get 291 kelvin.

01:11 I am given a pressure of 17 .2 atmospheres.

01:21 So i need to select a universal gas constant, or in other words, r.

01:26 We have a couple of options to choose from.

01:29 The constant is the same, but it looks a little different based upon what units it is recorded in.

01:34 So i would like to use the r that is in atmospheres, since my pressure is in atmospheres.

01:40 So that r value is 0 .0 821 liters times atmospheres over mole times kelvin.

01:54 It's very important for us to write all of these units in because in a few minutes we're going to look at how they cancel leaving only the unit leaders for this problem.

02:05 All right, we are ready to plug information in...

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