40.0g of K reacts with 40.0g of Cl_(2) to form KCl. Which is the limiting reagent? 2K(s)+Cl_(2)(g)arrow 2KCl(s) Cl_(2) KCI K 13 points

Question

Answer 1

## Step 1: Determine Molar MassFind the molar masses of each reactant:-

(Potassium) has a molar mass of

-

(Chlorine gas) has a molar mass of

## Step 2: Calculate Moles of Each ReactantConvert the given masses to moles:

## Step 3: Determine Stoichiometric RatiosFrom the balanced equation:

The ratio required by the reaction is:

## Step 4: Compare Available RatiosCompare the mole ratio of the available reactants to the stoichiometric ratio:

Calculate the limiting reagent:

Since we only have

but need

,

is less than required, making

the limiting reagent.

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