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}=(4g)/(58.44g/mole)=0.068moles`

`\text{Moles of }AgNO_3=\frac{\text{Mass of }AgNO_3}{\text{Molar mass of }AgNO_3}=(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`