Zinc metal reacts with aqueous silver nitrate to produce...

Zinc metal reacts with aqueous silver nitrate to produce silver metal and aqueous zinc nitrate according to the following equation (unbalanced): $$ \mathrm{Zn}(s)+\mathrm{AgNO}_{3}(a q) \longrightarrow \operatorname{Ag}(s)+\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(a q) $$ What mass of silver metal is produced when $25.00 \mathrm{~g}$ Zn is added to a beaker containing $105.5 \mathrm{~g} \mathrm{AgNO}_{3}$ dissolved in $250 \mathrm{~mL}$ of water. Determine the mass amounts of each substance present in the beaker when the reaction is complete.

Zinc metal reacts with aqueous silver nitrate to produce silver metal and aqueous zinc nitrate according to the following equation (unbalanced):
$$
\mathrm{Zn}(s)+\mathrm{AgNO}_{3}(a q) \longrightarrow \operatorname{Ag}(s)+\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(a q)
$$
What mass of silver metal is produced when $25.00 \mathrm{~g}$ Zn is added to a beaker containing $105.5 \mathrm{~g} \mathrm{AgNO}_{3}$ dissolved in $250 \mathrm{~mL}$ of water. Determine the mass amounts of each substance present in the beaker when the reaction is complete.

Key Concepts

Stoichiometry

Stoichiometry involves using a balanced chemical equation to relate the moles of reactants and products in a chemical reaction. It allows one to convert between masses and moles, determine the quantities of substances involved, and calculate theoretical yields.

Limiting Reactant

The concept of the limiting reactant is critical in chemical reactions because it is the substance that is entirely consumed first, thereby limiting the maximum amount of product that can be formed. Determining the limiting reactant involves comparing the mole ratios of the reactants present to those required by the balanced equation.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. It serves as a conversion factor between the mass of a substance and the number of moles, facilitating stoichiometric calculations.

Conservation of Mass

The principle of conservation of mass states that mass is neither created nor destroyed during a chemical reaction. This concept ensures that the total mass of the reactants equals the total mass of the products, which is fundamental when accounting for all substances present after a reaction.

Transcript

00:01 We're told that zinc metal reacts with silver nitrate to produce silver metal and aqueous zinc nitrate solution.

00:07 We're given the equation of the reaction.

00:10 It's a single replacement equation of hno3 and we have znno3 bracket 2 plus ag.

00:25 Because we're going to have to balance this this is balanced now.

00:31 Now we're told what mass of silver will be produced when 25 grams of zinc is added to a beaker containing 105 .5 grams of zinc nitrate dissolved in 250 mls of water.

00:50 So what this means is that first we can find the concentration of the zinc nitrate, find the moles of that and find the number of moles of the zinc we're given.

01:00 So we have to first determine which of them is the limiting reagent.

01:06 So what i'm going to say, what we have to do is find the number of moles of the zinc that was given to us would have been 25 divided by the relative atomic mass of zinc which is 25 .00 which is 65 .38 and when you divide this you have 0 .38 moles.

01:37 Well the number of moles of the silver nitrate that we were provided with would have been the mass which we were given as 105 .5 grams divided by the molar mass of silver nitrate is 169 .87.

02:00 And when you divide this you would have 0 .62 moles.

02:06 So these are the number of moles of the reactant.

02:11 Now we have to determine one of them is the limiting reactant.

02:14 Only one of them is completely used up.

02:17 And the only way we can deduce that is to try to find the number of moles of silver that is produced from each of them...

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