What is the pressure in torr that a 0.44-g sample of carbon dioxide gas will exert at a temperature of 46.2°C when it occupies a volume of 5.00 L?

Answer 1

#31.92#

To solve this problem we will use the ideal gas law equation:

#PV=nRT#
To find pressure we divided both sides by #V#
#(PcancelV)/cancelV=(nRT)/V#
#P=(nRT)/V#
First we need to convert the temperature to K so we add #212#
#46.2°C +212K=258.2K#
Now we also need to find the number of moles first we find the molar mass of #CO_2#, which is 44. We take our #.44# and divided by #44#.
#("gram sample of carbon dioxide")/("molar mass of " CO_2)#
#(.44 " grams")/(44 " Molar mass")=.01 " moles"#

Now we have:

#n=.01#
#R=0.0806# This is the universal gas constant
#T=258.2K#
#V=5.00L#

Let's plug it in:

#P=(.01"moles"(0.0806(Lxxatm)/(molxxK)(258.2K)))/(5.00L)#
#P=.042 " atm"#

To find the torr you multiply:

#.042xx760=31.92#
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Answer 2

The pressure exerted by the carbon dioxide gas is approximately 79.5 torr.

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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.

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.

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.

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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