Answer: Stochiometric coefficients
Explanation: The chemical equations must be balanced to follow the law of conservation of mass which says that the mass of products must be same as the mass of reactants.
This is a skeletal equation and needs to be balanced by adjusting the stochiometric coefficients. In order to keep the mass same, the number of atoms must be same on both sides.
The first step is to make a balanced chemical equation.
2AgNO3 + CaCl2 ---> 2AgCl + Ca(NO3)2
Molecular Weights:
CaCl2 = 110.98 g/mol
AgNO3 =170.01
AgCl: 143.45 g/mol
Volume:
CaCl2: 30.0mL=0.03L
AgNO3: 15.0mL=0.015 L
Solving for the limiting reactant one needs to get the mols CaCl2 and mols AgNO3:
CaCl2: 0.150M(mol/L) * 0.03L = 0.0045 moles
AgNO3: 0.100M*0.015L = 0.0015 moles
Since the stoichiometric ratio of AgNO3 to CaCl2 is 2:1
0.0015 mols AgNO3 *(1 mol CaCl2/ 2 mols AgNO3) = 0.00075 mols CaCl2
Since the answer is lesser than CaCl2 then the limiting reactant is AgNO3.
To get the mass of AgCl one will do a stoichiometric calculation with respect to the limiting reactant, AgNO3.
0.0015 moles AgNO3 *
Answer:
C
Explanation:
Ionic compounds consist of ions, which are formed when elements gain or lose electrons through donating or receiving.
Answer:
69.7% is percent yield
Explanation:
Based on the reaction:
3Ca(NO3)2(aq) + 2Na3PO4(aq) → Ca3(PO4)2(s) + 6NaNO3(aq)
2 moles of Na3PO4 react producing 6 moles of NaNO3.
As 24.2 moles of Na3PO4 react, theoretical moles of NaNO3 produced are:
24.2 moles Na3PO4 * (6 moles NaNO3 / 2 moles Na3PO4) =
72.6 moles of NaNO3
As there are produced 50.6 moles of NaNO3, percent yield is:
50.6 moles NaNO3 / 72.6 moles NaNO3 =
<h3>69.7% is percent yield</h3>