Question

34 litre of water vapours at stp are condensed to liquid state. The volume occupied by it is

Answer 1

Answer:

$Assuming the water vapour acts as an Ideal Gas:</p><p></p><p>The formula for an Ideal Gas is V = nRT/p or pV/(RT)=n</p><p></p><p>R is the ideal gas constant (~8.314 J/(mol*K).</p><p></p><p>Standard Pressure is 1.01*10⁵ Pa.</p><p></p><p>Wenn can now insert those numbers into the equation and get n=1.52 mole.</p><p></p><p>(This calculation can be done easier if you remember that 1 mole equals 22.414 litres at STP, you just need to divide 34 by 22.414)</p><p></p><p>With the amount of substance you can now calculate the mass of Water.</p><p></p><p>n*M=m</p><p></p><p>Molar Mass of Water is about 18 g/mol. (2*1 for Hydrogen and 16 for Oxygen)</p><p></p><p>1.52 mol * 18 g/mol equals 27.36 g.</p><p></p><p>Since the density is given as 1 g/ml the solution to your question is 27.4 ml.</p><p></p><p>(The exact solution would be 27.33 ml if you don't round the values and use the most exact values for R, p and M)</p><p></p><p>hope it will help u</p><p></p><p>$