What volume would be occupied by a #0.1mol# quantity of gas at a temperature of #310K#, and a pressure of #700mmHg#?

Answer 1

Well, #PV=nRT#.........and so.......#V~=3*L#

You must simply KNOW that #1*atm# pressure will support a column of mercury that is #760*mm# high; and thus #"Torr"-=1*mm*Hg# stands in for a pressure measurement. You must also know the relationship between #"degrees Kelvin"#, and #"degrees centigrade"#: #0# #""^@C-=+273.15*K#

#V=(nRT)/P=(0.1*molxx0.0821*(L*atm)/(K*mol)xx310*K)/((700*"Torr")/(760*"Torr"*atm^-1))#

#=??*L#. The question would have been better proposed had it been specified that #0.1*mol# quantity of gas had been enclosed in a piston at the given temperature and pressure.

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Answer 2

Olivia Anton

Use the Ideal Gas Law: (V = \frac{{nRT}}{{P}})

(V = \frac{{(0.1,mol) \cdot (0.0821,L,mol^{-1}K^{-1}) \cdot (310,K)}}{{(700,mm,Hg)}})
(V \approx 0.296,L)

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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.

What volume would be occupied by a #0.1*mol# quantity of gas at a temperature of #310*K#, and a pressure of #700*mm*Hg#?

What volume would be occupied by a #0.1mol# quantity of gas at a temperature of #310K#, and a pressure of #700mmHg#?