Calculate how many moles of products(s) would be produced if 0.500 mole of the first reactant were to react completely.
BaCl2 + 2AgNO3 --> 2AgCl +Ba(NO3)2
Use the coefficients. The ratios, as written, are 1:2:2:1
To calculate the moles of product produced, you need to use the stoichiometry of the balanced chemical equation. In this case, the balanced equation is:
BaCl2 + 2AgNO3 -> 2AgCl + Ba(NO3)2
According to the balanced equation, 1 mole of BaCl2 reacts with 2 moles of AgNO3 to produce 2 moles of AgCl and 1 mole of Ba(NO3)2.
Given that you have 0.500 moles of BaCl2, you can use the stoichiometry to calculate the moles of products formed.
1 mole of BaCl2 reacts with 2 moles of AgNO3, so for 0.500 moles of BaCl2:
0.500 moles BaCl2 x (2 moles AgNO3 / 1 mole BaCl2) = 1.000 moles AgNO3
Therefore, if 0.500 moles of BaCl2 were to react completely, 1.000 moles of AgNO3 would be consumed.
Similarly, since 1 mole of BaCl2 reacts with 2 moles of AgCl, the number of moles of AgCl produced would be twice the number of moles of AgNO3 consumed.
1.000 moles AgNO3 x (2 moles AgCl / 2 moles AgNO3) = 1.000 moles AgCl
Finally, we also have 0.500 moles of Ba(NO3)2 produced, as it has a 1:1 molar ratio with BaCl2.
Therefore, if 0.500 moles of BaCl2 were to react completely, you would get 1.000 moles of AgNO3, 1.000 moles of AgCl, and 0.500 moles of Ba(NO3)2 as products.