According to the following reaction, how many grams of copper(II) chloride are necessary to form 0.984 moles silver chloride?
silver nitrate (aq) + copper(II) chloride (s) silver chloride (s) + copper(II) nitrate (aq)
CuCl2 + 2AgNO3 ==> 2AgCl + Cu(NO3)2
Here is an example problem I've posted for simple stoichiometry.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the grams of copper(II) chloride required to form a specific number of moles of silver chloride, we need to use the balanced chemical equation and molar masses of the substances involved.
The balanced equation is:
2 AgNO3 (aq) + CuCl2 (s) → 2 AgCl (s) + Cu(NO3)2 (aq)
From the equation, we can see that 2 moles of AgNO3 react with 1 mole of CuCl2 to produce 2 moles of AgCl.
Since the molar mass of CuCl2 is approximately 134.45 g/mol, we can use the following proportion to find the grams of CuCl2:
1 mol CuCl2 / 2 mol AgCl = x g CuCl2 / 0.984 mol AgCl
Calculating:
x = (0.984 mol AgCl x 1 mol CuCl2/2 mol AgCl) x (134.45 g CuCl2/1 mol CuCl2)
x = 65.9 g CuCl2
Therefore, 65.9 grams of copper(II) chloride are necessary to form 0.984 moles of silver chloride.