The balanced equation for the above reaction is as follows;
2AgNO₃ + CaCl₂ ---> 2AgCl + Ca(NO₃)₂
stoichiometry of AgNO₃ to CaCl₂ is 2:1
we first need to find the limiting reactant
number of moles reacted = molarity x volume
number of AgNO₃ moles = 0.22 mol/L x 0.1050 L = 0.023 mol
number of CaCl₂ moles = 0.13 mol/L x 0.1050 L = 0.014 mol
according to molar ratio of 2:1
if we assume AgNO₃ to be the limiting reactant
if 2 mol of AgNO₃ react with 1 mol of CaCl₂
then 0.023 mol of AgNO₃ reacts with - 0.023/2 = 0.012 mol of CaCl₂
0.012 mol of CaCl₂ is required but 0.014 mol of CaCl₂ is required
therefore CaCl₂ is in excess and AgNO₃ is therefore the limiting reactant
the amount of products formed depends on the amount of limiting reactant present
stoichiometry of AgNO₃ to AgCl is 2:2
the number of moles of AgCl formed = number of AgNO₃ moles reacted
therefore number of AgCl moles formed = 0.023 mol
mass of AgCl formed = 0.023 mol x 143.3 g/mol = 3.3 g
mass of AgCl formed = 3.3 g
Be more specific, I could possibly find the asnwer you're looking towards.
Answer:
txt and I'm going out of the way for a bit but it will probably take 6th and 6th and then we will have a lot and we will have a lot and we will make it work and I'm not
You can easily find hundreds on the internet.
Each particular chemical reaction cannot be expected to occur at identical rates.
True. Not all chemical reactions happen at the same rate, depending on the catalyst.
