14 carbon dioxide gas 100 mole at 373 k occupies 536 ml at...

14. Carbon dioxide gas (1.00 mole) at 373 K occupies 536 mL at 45.0 atmospheres of pressure. a) What is the calculated value of the pressure using the Van der Waals equation? For CO2, a = 3.61 𝐿^2𝑎𝑡𝑚/𝑚𝑜𝑙^2 and b = 0.0428 𝐿/𝑚𝑜𝑙 b) By what percentage does this calculated value deviate from the real value?

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00:02 Hi, so we are to solve for the volume of the pressure using the vandervald's equation.

00:09 Vandervald's equation is pressure plus a n squared over v squared, then volume v minus n b is equivalent to n r t.

00:26 Now since we're solving for pressure, we can just rearrange this.

00:31 Will have n r t over volume minus n b minus a n squared over v squared okay so let's plug in the given values here the number of moles is 1 r is 0 .0821 liters a tm per mole kelvin the temperature is 373 kelvin the volume is 536 we have to convert this to liters because r is in terms of liters so a thousand of l is one liter minus the number of moles one mole b is we have b that's equivalent to 0 .0 4 to 8 liters per mole a is 3 .61 liter squared a tm per mole squared the number of moles is 1.

01:50 Volume is 536 over 1000.

01:54 Let's just write the answer for that.

01:56 536 divided by 1000 is 0 .536.

02:02 And this is liters.

02:05 Raise that to the power of 2.

02:08 Cancel some units.

02:10 You can cancel moles.

02:12 Kelvin.

02:14 Moles.

02:17 You can also cancel liters.

02:19 And here we can cancel liters.

02:22 Moles.