Q2. In a vacuum chamber of $0.01 \mathrm{~atm}$, the air is heated to $3000 \mathrm{~K}$. Determine convertion ratio of NO at chemical equilibrium state?
$$
\begin{array}{l}
\text { Air at } 0.01 \mathrm{~atm}, 3000 \mathrm{~K} \
\mathrm{O}_{2}+3.76 \mathrm{~N}_{2} \text { à } \mathrm{xNO}+(1-\mathrm{x} / 2) \mathrm{O}_{2}+ \
(3.76-\mathrm{x} / 2) \mathrm{N}_{2} \
\mathrm{x}=?
\end{array}
$$

Question

Q2. In a vacuum chamber of $0.01 \mathrm{~atm}$, the air is heated to $3000 \mathrm{~K}$. Determine convertion ratio of NO at chemical equilibrium state?
$$
\begin{array}{l}
\text { Air at } 0.01 \mathrm{~atm}, 3000 \mathrm{~K} \
\mathrm{O}_{2}+3.76 \mathrm{~N}_{2} \text { à } \mathrm{xNO}+(1-\mathrm{x} / 2) \mathrm{O}_{2}+ \
(3.76-\mathrm{x} / 2) \mathrm{N}_{2} \
\mathrm{x}=?
\end{array}
$$

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Write the balanced chemical equation**: The formation of NO from air components involves the reaction of nitrogen and oxygen. The balanced equation for the formation of NO is $N_2 + O_2 \rightarrow 2NO$. ‖ ‖ 2 ⋮ **Set up the equilibrium expression**: For the reaction $N_2 + O_2 \rightarrow 2NO$, the equilibrium constant expression is $K = \frac{[NO]^2}{[N_2][O_2]}$. ‖ ‖ 3 ⋮ **Express concentrations in terms of x**: Let x be the conversion ratio of NO at equilibrium. The initial moles of $O_2$ and $N_2$ are in the ratio of 1:3.76. At equilibrium, the moles of $NO$ will be $2x$, $O_2$ will be $1 - \frac{x}{2}$, and $N_2$ will be $3.76 - \frac{x}{2}$. ‖ ‖ 4 ⋮ **Apply the ideal gas law**: Since the reaction is in a vacuum chamber at $0.01 \mathrm{~atm}$ and $3000 \mathrm{~K}$, we can assume that the volume is constant and the partial pressures are proportional to the mole fractions. Thus, $P_{NO} = 2xP_{total}$, $P_{O_2} = (1 - \frac{x}{2})P_{total}$, and $P_{N_2} = (3.76 - \frac{x}{2})P_{total}$. ‖ ‖ 5 ⋮ **Calculate the equilibrium constant K**: The value of K for the formation of NO at $3000 \mathrm{~K}$ needs to be known or given to solve for x. Assuming K is known, we can substitute the partial pressures into the equilibrium expression to solve for x. ‖ ‖ 6 ⋮ **Solve for x**: Substitute the expressions for $P_{NO}$, $P_{O_2}$, and $P_{N_2}$ into the equilibrium constant expression and solve for x. This will require algebraic manipulation and possibly numerical methods if the equation is not easily solvable by hand. ‖ ∻Answer∻ ⚹ The conversion ratio of NO at chemical equilibrium state, x, is calculated by solving the equilibrium constant expression with the given conditions. The exact value of x depends on the known value of the equilibrium constant K at $3000 \mathrm{~K}$. ⚹ ∻Key Concept∻ ⚹ Equilibrium constant expression ⚹ ∻Explanation∻ ⚹ The conversion ratio of NO at equilibrium can be determined by using the equilibrium constant expression, which relates the partial pressures of the reactants and products at equilibrium. ⚹◊How does the temperature affect the conversion ratio of NO in a chemical equilibrium state at different pressures?⍭ Generate me a similar question◊

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