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If 5.00 g of MgCl2 and 5.00 g of AgNO3 are allowed to react, how many grams of AgCl would be produced?

b) Which reactant is not totally consumed by the reaction? How much remains (g)?

Answer :

Final answer:

The question involves a chemical reaction between magnesium chloride and silver nitrate where AgCl is produced and foreseeing which reactant is in excess. The solution lies in understanding the principles of stoichiometry, which reveals that AgNO3 is the limiting reactant and MgCl2 is in excess.

Explanation:

The subject of your question involves a chemical reaction between magnesium chloride (MgCl2) and silver nitrate (AgNO3). The reaction would look like this:

MgCl2 + 2 AgNO3 -> 2 AgCl + Mg(NO3)2

We need to determine how much AgCl can be formed from 5g of each reactant and which reactant is in excess. This problem involves understanding stoichiometry, which allows us to calculate the amounts of reactants and products in a chemical reaction.

First, let's calculate the molar mass of the reactants and product. Then determine how many moles are there in 5 g of each reactant. Since the reaction consumes AgNO3 and MgCl2 in a 2:1 ratio, it is AgNO3 that limits the reaction, as it gets consumed sooner.

The remaining quantity of MgCl2 can be determined by subtracting the amount of MgCl2 reacted.

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