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A sample of gas at 288.0K has a volume of 21 L and exerts a pressure .982 ATMs how many moles of gas are in the sample

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We can use the Ideal Gas Law to solve this problem:

PV = nRT

where P is pressure, V is volume, n is the number of moles of gas, R is the gas constant (0.08206 L·atm/K·mol), and T is the temperature in Kelvin.

First, let's convert the pressure to units of atmospheres:

0.982 atm

Now, let's convert the volume to units of liters:

21 L

And let's convert the temperature to Kelvin by adding 273.15:

288.0 K + 273.15 = 561.15 K

Now we can plug these values into the Ideal Gas Law and solve for n:

PV = nRT

n = PV/RT

n = (0.982 atm) x (21 L) / (0.08206 L·atm/K·mol x 561.15 K)

n = 0.989 mol

Therefore, there are approximately 0.989 moles of gas in the sample.

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