Zinc metal reacts with silver nitrate according to the reaction:

zn(s) + 2agno3(aq)zn(no3 )2 (aq) + 2ag(s)

calculate the mass of ag that forms when 3.00g of zinc metal is placed in an aqueous solution containing 3.75g of silver nitrate?

2.38 grams of silver forms when 3.00g of zinc metal is placed in an aqueous solution containing 3.75g of silver nitrate.

Explanation:

To calculate the number of moles, we use the equation:

....(1)

The chemical equation is:

By stoichiometry of the reaction;

2 moles of silver nitrate reacts with 1 mole of zinc

Thus 0.0220 moles silver nitrate react with= moles of zinc

Thus silver nitrate will acts as limiting reagent and zinc acts as excess reagent.

2 moles of silver nitrate produces 2 mole of silver

Thus 0.0220 moles silver nitrate react with= moles of silver

Thus 2.38 grams of silver forms when 3.00g of zinc metal is placed in an aqueous solution containing 3.75g of silver nitrate.

the answer is true.

periodic trends is an atom that gets larger as the number of electronic shells increase, the radius of atoms increases as you go down a certain group in the periodic table of elements. in general, the size of an atom will decrease as you move from left to right of a certain period.