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C2.
A reversible reaction between hydrogen and iodine occurs as follows:
$\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \leftrightharpoons 2 \mathrm{HI}(\mathrm{g}) \quad \mathrm{K}_{\mathrm{c}}=49.0 \text { at } 700 \mathrm{~K}$
Where $\mathrm{K}_{c}$ is the equilibrium constant.
(a) If a $10 \mathrm{~L}$ reaction vessel is fed with $1 \mathrm{~mole}$ of $\mathrm{H}_{2}$ and $1 \mathrm{~mole}_{2}$ at $700 \mathrm{~K}$, calculate the equilibrium concentrations of all components?
(b) If $\mathrm{k}_{\mathrm{r}}=1.20 \times 10^{-3} \mathrm{M}^{-1} \mathrm{~s}^{-1}$ at $700 \mathrm{~K}$, determine the value of $\mathrm{k}_{\mathrm{t}}$ at the same temperature? Where $\mathrm{k}_{\mathrm{f}}$ is the forward reaction rate constant and $\mathrm{k}_{r}$ is the reverse rate constant.
(c) If the forward reaction is endothermic, explain with justification how an increase in temperature effects the values of $\mathrm{K}_{\mathrm{c}}, \mathrm{k}_{\mathrm{f}}$ and $\mathrm{k}_{\mathrm{r}}$ ?
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Answer from Sia

Posted 3 months ago

Solution

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1 Answer

[Insert equilibrium concentrations here]

Key Concept

Equilibrium concentrations are determined by applying the equilibrium constant to the changes in concentrations of reactants and products.

Explanation

The equilibrium constant expression relates the concentrations of reactants and products at equilibrium. By setting up a system of equations based on the stoichiometry of the reaction and the equilibrium constant, we can solve for the unknown concentrations.

Solution

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2 Answer

[Insert value of $k_r$ here]

Key Concept

The reverse rate constant can be calculated from the equilibrium constant and the forward rate constant.

Explanation

Knowing the equilibrium constant and the forward rate constant allows us to find the reverse rate constant by rearranging the relationship between these constants.

Solution

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3 Answer

An increase in temperature will increase $K_c$, $k_f$, and $k_r$, with a more significant increase in $k_f$ for an endothermic reaction.

Key Concept

Temperature changes affect equilibrium constants and rate constants differently depending on the endothermic or exothermic nature of the reaction.

Explanation

For an endothermic reaction, increasing temperature shifts the equilibrium towards products, increasing $K_c$. The rate constants $k_f$ and $k_r$ also increase with temperature, but the forward rate constant increases more due to the reaction absorbing heat.

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