2.00 L of 18.5 M H2SO4, concentrated sulfuric acid Q. 2 Calculate the number of moles and the mass of the solute in each of the following

Mass = 3626 g

Number of moles = 37 mol

Explanation:

Given data:

Volume of solution = 2.00 L

Molarity of solution = 18.5 M

Number of moles of solute  = ?

Mass of solute = ?

Solution:

Molarity = number of moles / volume in L

By putting values,

18.5 M = number of moles / 2.00 L

Number of moles = 18.5 M × 2 L

Number of moles = 37 mol

Mass of solute:

Mass = number of mole × molar mass

Mass = 37 mol × 98 g/mol

Mass = 3626 g

a  solution  is always transparent, light passes through with no scattering from solute particles which are molecule in size. the  solution  is homogeneous and does not settle out. a colloid is intermediate between asolution  and a  suspension. while asuspension  will separate out a colloid will not.

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml