How many moles of carbon monoxide must be placed into a 40.0-L tank to develop a pressure of 965

step 1 Hello. This appears to be another ideal gas law equation problem. So we're going to need the ide

How many moles of carbon monoxide must be placed into a...

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Key Concepts

Ideal Gas Law

The ideal gas law is a fundamental equation relating pressure, volume, temperature, and the number of moles (PV = nRT). It is widely used to solve problems involving gases under conditions where they behave ideally, providing a connection between macroscopic measurements and the microscopic amount of substance present.

Unit Conversion for Pressure and Temperature

Accurate calculations using the ideal gas law require all quantities to be in the correct units. This often involves converting pressure (for example, from torr to atmospheres) and temperature (from degrees Celsius to Kelvin) so that they are compatible with the value of the gas constant used in the equation.

Gas Constant (R)

The gas constant is a key numerical factor in the ideal gas law that links pressure, volume, temperature, and moles. Its value depends on the units used in the problem (commonly 0.0821 L·atm·K?¹·mol?¹ when pressure is in atmospheres and volume in liters), ensuring that the equation remains dimensionally consistent.

Transcript

00:01 Hello.

00:03 This appears to be another ideal gas law equation problem.

00:08 So we're going to need the ideal gas law equation, which is pv equals nrt.

00:21 Reading through the problem, i see that we are trying to solve for moles.

00:26 We want to know how many moles of carbon dioxide.

00:40 Reading on through the problem some more, we see that we are given a volume.

00:44 The container size is 40 liters.

00:50 We are given a pressure.

00:53 That pressure is in tor.

00:54 It is 965 tor.

01:02 Temperature.

01:03 Given a temperature in celsius.

01:06 18 degrees celsius.

01:12 And we know that for any gas law problem, temperature has to be in kelvin.

01:16 So before i go any further, i'm going to go ahead and multiply this by 273 to convert this to 291 kelvin.

01:27 The only thing i am missing here now is a value for the universal gas constant.

01:33 So we have a couple of those we can select between.

01:35 I'm going to select the one that has tor in it because the pressure in this problem is in tor.

01:42 So the r that i'm going to use is 62 .4 liters times tor divided by mole over kelvin, mole times kelvin rather.

02:01 So now we have all of our values for our pv equals nrt equation...

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