Q. \(2\text{so}_2(g) + \text{o}_2(g) \rightarrow 2\text{so}_3(g)\).

Q: What is the balanced equation for \mathrm{2SO_2 + O_2 \to 2SO_3} ?

It is already balanced: \mathrm{S} : 2\to2, \mathrm{O} : 4+2=6\to2\times3=6.

Q: What is the reaction stoichiometric ratio among \mathrm{SO_2} , \mathrm{O_2} , and \mathrm{SO_3} ?

\mathrm{2\ SO_2 : 1\ O_2 : 2\ SO_3} . Use coefficients directly for mole conversions.

Q: How do I determine the limiting reactant if given masses of \mathrm{SO_2} and \mathrm{O_2} ?

Convert each mass to moles, then compare using \mathrm{moles\ O_2 / moles\ SO_2} to the required ratio 1/2. Smaller ratio implies limiting reactant.

Q: How do I calculate the theoretical yield of \mathrm{SO_3} from a given amount of \mathrm{SO_2} ?

Convert \mathrm{SO_2} mass to moles. Use 2\ \mathrm{SO_2}\to2\ \mathrm{SO_3}, so moles \mathrm{SO_3}= moles \mathrm{SO_2}. Then convert moles to grams using molar mass.

Q: How do I compute \Delta n_g and its effect on K_p for \mathrm{2SO_2 + O_2 \to 2SO_3} ?

\Delta n_g = (2)-(2+1) = -1 . Negative \Delta n_g means higher pressure favors products, and \mathrm{K_p} is typically larger when favorable thermodynamically.

Answer

BALANCING

Let the coefficients be \(a\), \(b\), and \(c\):

\[
a\text{ SO}_2(g)+ b\text{ O}_2(g)\rightarrow c\text{ SO}_3(g)
\]

Balance sulfur first:

\[
a=c
\]

Balance oxygen next. Left side has \(2a\) O from \(\text{SO}_2\) plus \(2b\) O from \(\text{O}_2\). Right side has \(3c\) O from \(\text{SO}_3\).

\[
2a+2b=3c
\]

Substitute \(c=a\):

\[
2a+2b=3a \Rightarrow 2b=a
\]

Choose the smallest integers: take \(a=2\). Then \(b=1\) and \(c=2\).

Final balanced equation:

\[
2\text{ SO}_2(g)+ \text{ O}_2(g)\rightarrow 2\text{ SO}_3(g)
\]

Detailed Explanation

Goal: Balance the chemical equation

\[ \text{2SO}_2(g) + \text{O}_2(g) \rightarrow \text{2SO}_3(g) \]

Step 1: Identify the species in the equation.

The reactants are:

\(\text{SO}_2(g)\)
\(\text{O}_2(g)\)

The product is:

\(\text{SO}_3(g)\)

Step 2: List the coefficients shown in the given equation.

The equation already provides coefficients:

\(\text{2SO}_2(g)\) has coefficient \(2\)
\(\text{O}_2(g)\) has coefficient \(1\) (implied)
\(\text{2SO}_3(g)\) has coefficient \(2\)

Step 3: Check atom balance for sulfur (S).

Count sulfur atoms on the reactant side:

\(\text{2SO}_2\) contains \(2 \times 1 = 2\) sulfur atoms
\(\text{O}_2\) contains \(0\) sulfur atoms

Total sulfur on reactants:

\[ 2 \]

Count sulfur atoms on the product side:

\(\text{2SO}_3\) contains \(2 \times 1 = 2\) sulfur atoms

Total sulfur on products:

\[ 2 \]

Conclusion for sulfur: Sulfur is balanced.

Step 4: Check atom balance for oxygen (O).

Count oxygen atoms on the reactant side:

\(\text{2SO}_2\) has \(2 \times 2 = 4\) oxygen atoms
\(\text{O}_2\) has \(1 \times 2 = 2\) oxygen atoms

Total oxygen on reactants:

\[ 4 + 2 = 6 \]

Count oxygen atoms on the product side:

\(\text{2SO}_3\) has \(2 \times 3 = 6\) oxygen atoms

Total oxygen on products:

\[ 6 \]

Conclusion for oxygen: Oxygen is balanced.

Step 5: State the balanced equation.

Since both sulfur and oxygen are balanced, the given equation is already balanced:

\[ \text{2SO}_2(g) + \text{O}_2(g) \rightarrow \text{2SO}_3(g) \]

See full solution

Need help solving chemistry? Try our AI homework tools!

Homework helper

General Chemistry FAQs

What is the balanced equation for \( \mathrm{2SO_2 + O_2 \to 2SO_3} \)?

It is already balanced: \( \mathrm{S} \): \(2\to2\), \( \mathrm{O} \): \(4+2=6\to2\times3=6\).

What is the reaction stoichiometric ratio among \( \mathrm{SO_2} \), \( \mathrm{O_2} \), and \( \mathrm{SO_3} \)?

\( \mathrm{2\ SO_2 : 1\ O_2 : 2\ SO_3} \). Use coefficients directly for mole conversions.

How do I determine the limiting reactant if given masses of \( \mathrm{SO_2} \) and \( \mathrm{O_2} \)?

Convert each mass to moles, then compare using \( \mathrm{moles\ O_2 / moles\ SO_2} \) to the required ratio \(1/2\). Smaller ratio implies limiting reactant.

How do I calculate the theoretical yield of \( \mathrm{SO_3} \) from a given amount of \( \mathrm{SO_2} \)?

Convert \( \mathrm{SO_2} \) mass to moles. Use \(2\ \mathrm{SO_2}\to2\ \mathrm{SO_3}\), so moles \( \mathrm{SO_3}=\) moles \( \mathrm{SO_2}\). Then convert moles to grams using molar mass.

How do I compute \( \Delta n_g \) and its effect on \(K_p\) for \( \mathrm{2SO_2 + O_2 \to 2SO_3} \)?

\( \Delta n_g = (2)-(2+1) = -1 \). Negative \( \Delta n_g \) means higher pressure favors products, and \( \mathrm{K_p} \) is typically larger when favorable thermodynamically.

What is the expression for the equilibrium constant \(K_c\) for this reaction? Assume equilibrium concentrations.

\( \displaystyle K_c=\frac{[\mathrm{SO_3}]^2}{[\mathrm{SO_2}]^2[\mathrm{O_2}]}\). Use equilibrium concentrations only.

Use AI to balance the equation.
Stepwise math help for stoichiometry.

301,983+ active customers
Analytical, General, Biochemistry, etc.

Organic Chemistry Solver Chemistry AI Science AI Solver