Sulfur dioxide reacts with chlorine to produce thionyl chloride.
[tex]SO_2(g)+2 Cl_2(g) \rightarrow SOCl_2(g)+ Cl _2 O ( g )[/tex]
If 0.400 mol of [tex]Cl _2[/tex] reacts with excess [tex]SO _2[/tex], how many moles of [tex]Cl _2 O[/tex] are formed?
A. 0.400 mol
B. 0.200 mol
C. 0.0500 mol
D. 0.100 mol
E. 0.800 mol
Answer (1)
The balanced chemical equation shows that 2 moles of C l 2 produce 1 mole of C l 2 O .
Use the molar ratio to set up a proportion: 2 e wl in e m o l e wl in e C l 2 1 e wl in e m o l e wl in e C l 2 O .
Multiply the proportion by the given moles of C l 2 (0.400 mol) to find the moles of C l 2 O formed.
Calculate the moles of C l 2 O : 0.400 e wl in e m o l e wl in e C l 2 × 2 e wl in e m o l e wl in e C l 2 1 e wl in e m o l e wl in e C l 2 O = 0.200 e wl in e m o l . The final answer is 0.200 m o l .
Explanation
Analyze the balanced equation The balanced chemical equation is: S O 2 ( g ) + 2 C l 2 ( g ) → SOC l 2 ( g ) + C l 2 O ( g ) . This equation tells us the ratio in which the reactants combine and the products are formed.
Identify the molar ratio From the balanced equation, we can see that 2 moles of C l 2 react to produce 1 mole of C l 2 O . This is a crucial piece of information for solving the problem.
Use the given information We are given that 0.400 mol of C l 2 reacts. We can use the molar ratio to find out how many moles of C l 2 O are formed.
Calculate moles of product To find the moles of C l 2 O formed, we can set up a proportion: m o l ese wl in eo f e wl in e C l 2 m o l ese wl in eo f e wl in e C l 2 O = 2 e wl in e m o l e wl in e C l 2 1 e wl in e m o l e wl in e C l 2 O m o l ese wl in eo f e wl in e C l 2 O = 2 e wl in e m o l e wl in e C l 2 1 e wl in e m o l e wl in e C l 2 O × 0.400 e wl in e m o l e wl in e C l 2 m o l ese wl in eo f e wl in e C l 2 O = 0.200 e wl in e m o l
State the final answer Therefore, 0.200 mol of C l 2 O are formed when 0.400 mol of C l 2 reacts with excess S O 2 .
Examples
In chemical manufacturing, understanding stoichiometry is crucial for optimizing reactions and minimizing waste. For instance, if you're producing C l 2 O , knowing the exact amount of C l 2 needed ensures efficient production and reduces the cost of unused reactants. This principle applies to various industrial processes, from pharmaceuticals to material science, where precise control over chemical reactions is essential for quality and economic efficiency.
