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# If 20 g of $CaC{O_3}$ is treated with 20 g of $HCl$ , how many grams of can be generated $C{O_2}$ according to the following equation?$CaC{O_3} + 2HCl \to CaC{l_2} + {H_2}O + C{O_2}$(Molecular masses: $CaC{O_3}$=100u, $HCl$=36.5u, $C{O_2}$=44u)  Hint: We can easily find the total amount of $C{O_2}$ gas generated by just finding out the limiting reagent in the reaction $CaC{O_3} + 2HCl \to CaC{l_2} + {H_2}O + C{O_2}$.

Complete step by step solution:
In order to calculate the total amount of $C{O_2}$ gas generated in the balanced chemical reaction $CaC{O_3} + 2HCl \to CaC{l_2} + {H_2}O + C{O_2}$ following steps have to be followed:
Step 1: First, we will convert the given amounts into moles.
Mass of $CaC{O_3}$ given = 20 g
Moles of $CaC{O_3}$ $= \dfrac{{{\text{mass of }}CaC\mathop O\nolimits_3 }}{{{\text{molecular mass of}}CaC\mathop O\nolimits_3 }} = \dfrac{{20}}{{100}} = 0.2$.
Mass of $HCl$ given = 20 g
Moles of $HCl$$= \dfrac{{20}}{{36.5}} = 0.547$.
Step 2: In this step we have to identify limiting reagent.
Limiting reagent is defined as those substances which get completely consumed in a chemical reaction. They also govern the quantity of the final product of a chemical reaction.
From the above balanced equation, we can say that 1 mol of $CaC{O_3}$ reacts with 2 mol of $HCl$.
Therefore, 0.2 mol of $CaC{O_3}$ will react with 0.4 mol of $HCl$.
As, we have 0.547 of $HCl$, hence $CaC{O_3}$ is the limiting reagent and $HCl$ is the excessive reagent
Step 3: In this last step, we will calculate the amount of $C{O_2}$ formed
As the amount of product formed depends on limiting reagent, hence, we can calculate amount of $C{O_2}$ formed as follows : 1 mol of $CaC{O_3}$ form $C{O_2}$= 1mol
Therefore, 0.2 mol of $CaC{O_3}$ will form $C{O_2}$ =$1 \times 0.2 = 0.2$$mol$.
Since, molecular mass of $C{O_2}$ is 44 u
Therefore, the mass of $C{O_2}$ formed $= {\text{ }}0.2 \times 44 =$$8.8{\text{ }}g$.

Note: It should be remembered that the chemical reaction should be balanced while finding limiting reagent. Also, the amount of product form in a chemical reaction is limited by limiting reagent.
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