The reaction of magnesium chloride with silver nitrate gives a precipitate of silver chloride. MgCl2(aq) + 2AgNO3(aq) + Mg(NO3)2(aq) + 2AgCl(s)
A solution containing 0.001 mol of magnesium chloride reacts with excess silver nitrate.
What is the mass of the precipitate formed?
[Molar mass/gmol-': AgCl = 143.4]
A 0.0729
B 0.1439
C 0.287g
D 0.574g
(Total for Question 5 = 1 mark)

Mass = 0.287 g

Explanation:

Given data:

Number of moles of MgCl₂ = 0.001 mol

Mass of precipitate formed (AgCl) = ?

Solution:

Chemical equation:

MgCl₂(aq) + 2AgNO₃(aq)    →       Mg(NO₃)₂(aq) + 2AgCl (s)

now we will compare the moles of MgCl₂ and AgCl.

            MgCl₂           :            AgCl

                1                :             2

           0.001             :       2/1×0.001 = 0.002

Mass of AgCl:

Mass = number of moles × molar mass

Mass = 0.002 mol × 143.4 g/mol

Mass = 0.287 g

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

i'm pretty sure it is letter c.) car