Suppose you have a 150.0 liter container that holds 12.5...

Suppose you have a 150.0 liter container that holds 12.5 moles of gas at a temperature of 300.0 °C, what is the pressure inside the container? (6 points) Given, R = 0.0821 (L x atm)/(Mole x K) or R = 62.4 (L x mm Hg)/(Mole x K)

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Transcript

00:02 Hi there.

00:03 In this question, we want to know the pressure.

00:09 When we are given the volume, we are also given the number of moles, and we are given the temperature.

00:23 So we want to know the pressure when we have a volume of 10 liters, number of moles of 2 .50, and a celsius temperature of 65.

00:38 More on that in a moment.

00:41 All right.

00:42 Well, if we have v and n, and t and we're trying to solve for p, this is an ideal gas law problem.

00:53 The ideal gas law tells us that pv, pressure times volume, is equal to n, which is the number of moles, times r, which is the universal gas constant, times temperature in kelvin.

01:06 Temperature must be in kelvin.

01:08 Well, in this question we're trying to solve for p, so let me divide both sides by volume.

01:14 That gives us pressure is equal to n -r -t over v.

01:22 Okay, so i am missing r here.

01:24 Let me add that.

01:26 And i'm going to use the one that has atmospheres in it, since the question doesn't specify what unit to put it in.

01:32 I will put it in atmospheres.

01:35 So that is 0 .0821 liters times atmospheres over mole times kelvin, reminding us that we need to convert our temperature to kelvin by adding 273 .15...

Question

Suppose you have a 150.0 liter container that holds 12.5 moles of gas at a temperature of 300.0 °C, what is the pressure inside the container? (6 points) Given, R = 0.0821 (L x atm)/(Mole x K) or R = 62.4 (L x mm Hg)/(Mole x K)

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