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.

b

explanation:

mitosis

they it depends on if one believes about radioactivity, they make a geiger counter beep but maybe it was going to beep anyway electronics do wierd things all the time or it was programmed to beep near certain metals.