Will you please explain this concept in more detail? Also, if you would, please

Question

Will you please explain this concept in more detail? Also, if you would, please show calculations using PV=nRT to explain. Thank you!

Remember the standard molar volume and learn howto use it with the ideal gas law. For instance, 2 moles of gas at O'C occupying 1.2 liters will have apressure of atm. To get this result, we start with the standard molar volume, 22.4 L, at STP First, the number of molco doublco, oo, according to the ideal gas law, the pressure doubles. Second, the volume is halved, so pressure doubles again.

Explanation / Answer

First let us calculate pressure using,

PV = nRT

rearranging,

P = nRT/V

feeding the values,

V = 11.2 L ; n = 2 moles ; R = gas constant ; T = 0 oC + 273.15 = 273.15 K

we get,

Pressure (P),

P = 2 x 0.08205 x 273.15/11.2

    = 4 atm

Using standard molar volume 22.4 L

Pressure is directly proportional to number of moles

P = n(RT/V)

So, 2 moles of gas would have double the pressure that it has when we half the moles.

Again, pressure is inversely related to volume,

P = (1/V)nRT

So, when the volume is halved, pressure would double.

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