Question

the illustration to the left represents a mixture of hydrogen ( light blue ) and iodine ( purple ) reacting to form a product. in the illustration: the product that forms is. the number of product molecules formed is. the limiting reagent is. the number of atoms/molecules in excess is.

Explanation:

Step1: Identify the reaction

Hydrogen ($H_2$) and iodine ($I_2$) react to form hydrogen - iodide ($HI$). The balanced chemical equation is $H_2 + I_2
ightarrow2HI$.

Step2: Count the reactant molecules

From the illustration, assume there are 3 $H_2$ molecules (light - blue) and 5 $I_2$ molecules (purple).

Step3: Determine the limiting reagent

According to the balanced equation, the mole ratio of $H_2$ to $I_2$ is 1:1. For 3 $H_2$ molecules, we need 3 $I_2$ molecules. Since we have 5 $I_2$ molecules, $H_2$ is the limiting reagent.

Step4: Calculate the number of product molecules

Since 1 molecule of $H_2$ forms 2 molecules of $HI$, 3 molecules of $H_2$ will form $2\times3 = 6$ molecules of $HI$.

Step5: Calculate the excess molecules

We used 3 $I_2$ molecules out of 5. So the number of $I_2$ molecules in excess is $5 - 3=2$.

Answer:

The product that forms is $HI$.
The number of product molecules formed is 6.
The limiting reagent is $H_2$.
The number of $I_2$ atoms/molecules in excess is 2.