How many moles, kmols in: 100 g of co2, 1 litre of ethyl alcohol of density 0.789 g/cm3 and a) 1.5m3 of o2 at 25°c and 1 atm. b) a mixture of water and ethyl alcohol is made up of 1 litre of water and 2.5 litre of alcohol. calculate the mass fraction and mol fraction for water and alcohol density of water 1000 kg/m density of alcohol 789 kg/m

Explanation:

1) Mass of carbon dioxide = 100 g

Molar mass of carbon dioxide = 44 g/mol

Moles of carbon dioxide =

1 mol = 0.001 kmol

2.273 moles= 2.273 × 0.001 kmol =

2) 1 liter of ethyl alcohol of density

Volume of ethyl alcohol ,V= 1 L = 1000 mL

Density of ethyl alcohol =d =

Mass of ethyl alcohol = m

Molar mass of  ethyl alcohol = 46 g/mol

Moles of ethyl alcohol =

3) Volume of oxygen gas,V =

Temperature of the gas = T= 25°C = 298.15 K

Pressure of the gas ,P= 1 atm

Moles of oxygen gas = n

0.01632 mol = 0.01632 × 0.001 kmol=

4) Volume water in mixture = 1 L

Density of water =  

Mass of water =

Volume of alcohol = 2.5 L

Density of alcohol =  

Mass of alcohol =

Mass of mixture = 1000 g + 1972.5 g = 2972.5 g

Mass percentage of water :

Mass percentage of alcohol :

Moles of water :

Moles of alcohol =

Mole fraction of water :

Mole fraction of alcohol :

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-