6. The following reaction scheme was allowed to reach chemical equilibrium:
$$
\mathrm{NOCl}(g) \rightleftharpoons \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \quad K_{c}=\left(4+\frac{w}{10}\right) \times 10^{-2} \text { at } 220^{\circ} \mathrm{C}
$$

Here
$w=$ the 7th digit of your URN
a) Initially the system contained no products and $5 \mathrm{M}$ of $\mathrm{NOCl}$. Find the equilibrium composition of the reactor.
b) Given an exothermic forward reaction explain how (and why) you could improve the production of $\mathrm{NO}(\mathrm{g})$ and $\mathrm{Cl}_{2}(g)$ (max 200 words)
c) Given that forward reaction is exothermic, explain with justification how an increase in temperature affects the values of $\mathrm{K}_{c}, \mathrm{k}_{f}$ and $\mathrm{k}_{r}$ ? (max 200 words)

Question

6. The following reaction scheme was allowed to reach chemical equilibrium:
$$
\mathrm{NOCl}(g) \rightleftharpoons \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \quad K_{c}=\left(4+\frac{w}{10}\right) \times 10^{-2} \text { at } 220^{\circ} \mathrm{C}
$$

Here
$w=$ the 7th digit of your URN
a) Initially the system contained no products and $5 \mathrm{M}$ of $\mathrm{NOCl}$. Find the equilibrium composition of the reactor.
b) Given an exothermic forward reaction explain how (and why) you could improve the production of $\mathrm{NO}(\mathrm{g})$ and $\mathrm{Cl}_{2}(g)$ (max 200 words)
c) Given that forward reaction is exothermic, explain with justification how an increase in temperature affects the values of $\mathrm{K}_{c}, \mathrm{k}_{f}$ and $\mathrm{k}_{r}$ ? (max 200 words)

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Set up the ICE table**: To find the equilibrium composition, we use an ICE (Initial, Change, Equilibrium) table. Initially, we have 5M of NOCl and 0M of NO and Cl₂. Let the change in concentration of NOCl be $-x$ and the formation of NO and Cl₂ be $+x$ each. ‖ ‖ 2 ⋮ **Write the equilibrium expression**: The equilibrium constant expression for the reaction is $K_c = \frac{[NO][Cl_2]}{[NOCl]}$. Substituting the equilibrium concentrations from the ICE table gives us $K_c = \frac{x^2}{5-x}$. ‖ ‖ 3 ⋮ **Calculate the equilibrium concentrations**: Given $K_c = (4 + \frac{w}{10}) imes 10^{-2}$, we solve for $x$ using the quadratic formula. This will give us the equilibrium concentrations of NOCl, NO, and Cl₂. ‖ ∻1 Answer∻ ⚹ [Insert calculated equilibrium concentrations here] ⚹ ∻Key Concept∻ ⚹ Chemical equilibrium and the use of ICE tables to find equilibrium concentrations ⚹ ∻Explanation∻ ⚹ The ICE table method allows us to express the changes in concentration of reactants and products in terms of a single variable, $x$, which we can solve for using the equilibrium constant. ⚹ ∻Solution∻ ‖ 1 ⋮ **Understand Le Chatelier's Principle**: To improve the production of NO and Cl₂, we can apply Le Chatelier's Principle, which states that a system at equilibrium will adjust to counteract any imposed change. ‖ ‖ 2 ⋮ **Apply changes to the system**: Since the forward reaction is exothermic, decreasing the temperature will shift the equilibrium to the right, producing more NO and Cl₂. Removing the products as they are formed will also shift the equilibrium to the right. ‖ ∻2 Answer∻ ⚹ Decrease temperature and remove products to improve production of NO and Cl₂ ⚹ ∻Key Concept∻ ⚹ Le Chatelier's Principle and its application to chemical equilibria ⚹ ∻Explanation∻ ⚹ By decreasing temperature and removing products, we can shift the equilibrium towards the products in an exothermic reaction, increasing their production. ⚹ ∻Solution∻ ‖ 1 ⋮ **Relate temperature to equilibrium constants**: An increase in temperature for an exothermic reaction will decrease the value of $K_c$ due to Le Chatelier's Principle. ‖ ‖ 2 ⋮ **Understand the effect on rate constants**: The Arrhenius equation shows that as temperature increases, the rate constants for both the forward and reverse reactions ($k_f$ and $k_r$) will increase, but $k_r$ will increase more for an exothermic reaction. ‖ ∻3 Answer∻ ⚹ Increase in temperature decreases $K_c$, increases both $k_f$ and $k_r$, but $k_r$ increases more ⚹ ∻Key Concept∻ ⚹ Temperature's effect on equilibrium constants and rate constants ⚹ ∻Explanation∻ ⚹ For exothermic reactions, increasing temperature decreases the equilibrium constant and increases the rate constants, with a greater increase in the reverse rate constant. ⚹◊What is the formula to calculate the equilibrium constant Kc for a reversible reaction?⍭ Generate me a similar question◊

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