Consider 2.00 moles of Argon, considered an Ideal Gas, at a density of 5.00 g/L

Question

Consider 2.00 moles of Argon, considered an Ideal Gas, at a density of 5.00 g/L and a pressure of 2.00 atm. What is the closest value to the temperature of this gas?

195 K          

I think I am doing something wrong since I am using the PV=nRT equation, so

2.00 atm (5.00g/L)=2.00(.08206)T so

10= (.16142)T

10/.16142 = 61.9 so the closest answer is 61 K.

However it says the answer is wrong, someone please help!

195 K          

I think I am doing something wrong since I am using the PV=nRT equation, so

2.00 atm (5.00g/L)=2.00(.08206)T so

10= (.16142)T

10/.16142 = 61.9 so the closest answer is 61 K.

However it says the answer is wrong, someone please help!

Explanation / Answer

B. 137 K

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