Which of the following statements is correct?

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(A) Statement $A$ is correct: At chemical equilibrium,the rate of the forward reaction equals the rate of the backward reaction,leading to constant co

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At equilibrium,the concentration of reactants and products becomes constant because the forward and backward reactions continue at the same rate,not because they cease.

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(A) Statement $A$ is correct: At chemical equilibrium,the rate of the forward reaction equals the rate of the backward reaction,leading to constant concentrations of reactants and products,even though the reactions do not stop.Statement $B$ is correct: $A$ catalyst provides an alternative pathway with lower activation energy,increasing the rates of both forward and backward reactions equally.Statement $C$ is correct: According to Le Chatelier's principle,for an exothermic reaction,increasing the temperature shifts the equilibrium to the left,decreasing the equilibrium constant $(K)$.Note: In many contexts,this question might be a multiple-correct type. However,if forced to choose the most fundamental definition,$A$ is the primary characteristic of equilibrium.

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For the reaction $CH_4(g) + 2O_2(g) \rightleftharpoons CO_2(g) + 2H_2O(l)$,the enthalpy change is $\Delta H_r = -170.8 \, kJ \, mol^{-1}$. Which of the following statements is $NOT$ true?

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The total pressure when both the solids dissociate simultaneously is:

$5 \ \text{moles}$ of $SO_2$ and $5 \ \text{moles}$ of $O_2$ are allowed to react to form $SO_3$ in a closed vessel. At the equilibrium stage,$60\%$ of $SO_2$ is used up. The total number of moles of $SO_2$,$O_2$,and $SO_3$ in the vessel now is:

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