Question

If 4.00 g of NaCl react with 10.00 g of AgNO3, what is the excess reactant?
AgCl

Answer 1

NaCl Would be the excess reactant, hope this helps :).

Answer 2

Answer : The excess reagent is, $NaCl$

Explanation : Given,

Mass of NaCl = 4 g

Mass of $AgNO_3$ = 10 g

Molar mass of NaCl = 58.44 g/mole

Molar mass of $AgNO_3$ = 169.87 g/mole

First we have to calculate the moles of $NaCl$ and $AgNO_3$.

$\text{Moles of }NaCl=\frac{\text{Mass of }NaCl}{\text{Molar mass of }NaCl}=\frac{4g}{58.44g/mole}=0.068moles$

$\text{Moles of }AgNO_3=\frac{\text{Mass of }AgNO_3}{\text{Molar mass of }AgNO_3}=\frac{10g}{169.87g/mole}=0.059moles$

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

$NaCl+AgNO_3\rightarrow NaNO_3+AgCl$

From the balanced reaction we conclude that

As, 1 moles of $AgNO_3$ react with 1 mole of $NaCl$

So, 0.059 moles of $AgNO_3$ react with 0.059 mole of $NaCl$

From this we conclude that, $NaCl$ is an excess reagent because the given moles are greater than the required moles and $AgNO_3$ is a limiting reagent and it limits the formation of product.

Hence the excess reagent is, $NaCl$