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What is the molar quantity of a sample of chlorine gas at #88# #""^@C# that exerts a pressure of #538mmHg#, and occupies a volume of #8.16*L#?

Answer 1

Mateo Aguilar

#"Moles of"# #Cl_2~=0.20*mol#

We use the Ideal Gas equation, and we know that #760*mm*Hg-=1*atm#.

And thus #n=(PV)/(RT)#

#=((538*mm*Hg)/(760*mm*Hg*atm^-1)xx8.16*L)/(0.0821*L*atm*K^-1*mol^-1xx361*K)#

#=??*mol#

What is the mass of this molar quantity of chlorine gas......?

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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What is the molar quantity of a sample of chlorine gas at #88# #""^@C# that exerts a pressure of #538*mm*Hg#, and occupies a volume of #8.16*L#?

What is the molar quantity of a sample of chlorine gas at #88# #""^@C# that exerts a pressure of #538mmHg#, and occupies a volume of #8.16*L#?