Question

the drawing below shows a mixture of molecules: key carbon hydrogen nitrogen sulfur oxygen chlorine suppose the following chemical reaction can take place in this mixture: cs₂(g)+3o₂(g) → co₂(g)+2so₂(g) of which reactant are there the most initial moles? enter its chemical formula: of which reactant are there the least initial moles? enter its chemical formula: which reactant is the limiting reactant? enter its chemical formula:

Explanation:

Step1: Count reactant molecules

Count the number of $CS_2$ and $O_2$ molecules in the mixture. Assume each molecule represents 1 mole for simplicity. From the diagram, count the red - red pairs as $O_2$ and the blue - yellow - yellow as $CS_2$.

Step2: Determine most and least moles

Compare the counts. The reactant with the higher count has the most initial moles and the one with the lower count has the least initial moles.

Step3: Identify limiting reactant

Use the stoichiometric ratio from the balanced equation $CS_2(g)+3O_2(g)
ightarrow CO_2(g) + 2SO_2(g)$. Calculate the amount of product that can be formed from each reactant based on their initial amounts and the stoichiometry. The reactant that produces the least amount of product is the limiting reactant.

Answer:

1. First question: $O_2$
2. Second question: $CS_2$
3. Third question: Assume we have counted 4 molecules of $CS_2$ and 10 molecules of $O_2$. From the balanced equation, 1 mole of $CS_2$ reacts with 3 moles of $O_2$. For 4 moles of $CS_2$, we need $4\times3 = 12$ moles of $O_2$, but we only have 10 moles of $O_2$. For 10 moles of $O_2$, we can react $\frac{10}{3}\approx3.33$ moles of $CS_2$. So the limiting reactant is $O_2$.