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The molar volume of a gas at STP, in liters, is ___ .
You can use the molar volume to convert 2 mol of any gas to ___ L.
You can also use the molar volume to convert 11.2 L of any gas to ____ mol. Avogadro’s law tells you that 1.2 L of O2(g) and 1.2 L of NO2(g) are ______-numbers of moles of gas.

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The   molar  volume  of  a  gas  at STP  in  liters   is  22.4 L 

 2mol  of  any  gas=  2  x  22.4l  =  44.8L

11.2  L  of any  gas  in  moles  is  calculated  as  follows
  1mole =22.4  L  what  about  11.2  L
(11,2  x1) /22.4 L  =  0.5 moles

1 mole  of  a  gas  =  22.4 L ,  what  about  1.2  L
that  is ( 1 x1.2L) /22.4 L  =0.054moles

Let us consider the following points

a) The volume of one mole of an ideal gas at STP (273.15 K and 1 atm) is 22.4 L.

b) the number of moles of in any given volume of gas can be calculated as:

[tex]Moles=\frac{22.4L}{Volumegiven}[/tex]

Solutions:

1) The molar volume of a gas at STP, in liters, is 22.4 L.

2) You can use the molar volume to convert 2 mol of any gas to 44.8 L

Volume = moles X 22.4L

Volume = 2 X 22.4 = 44.8L

3) You can also use the molar volume to convert 11.2 L of any gas to 0.5 mol.

As mentioned above

[tex]mole=\frac{volume}{22.4}=\frac{11.2}{22.4}=0.5mol[/tex]

4)  Avogadro’s law tells you that 1.2 L of O2(g) and 1.2 L of NO2(g) are ______-numbers of moles of gas.

The moles of oxygen will be:

[tex]mole=\frac{volume}{22.4}=\frac{1.2}{22.4}=0.0536mol[/tex]

The moles of nitrogen dioxide will be:

[tex]mole=\frac{volume}{22.4}=\frac{1.2}{22.4}=0.0536mol[/tex]

Total moles = 0.0536+0.0536 = 0.1072 moles


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