Question

for the reaction: x + 3y ⇌ 2z, the concentrations of these reactants and products are plotted versus time as the reaction progresses. these plots are labeled a - c. regions pertaining to the progress of the reaction are labeled d - g. using the information above, which of the following statements is/are true? i. the graph labeled a represents the change in the concentration of compound x as the reaction progresses. ii. the graph labeled c represents the change in the concentration of compound x as the reaction progresses. iii. the region e - f represents where the reaction is at equilibrium. iv. the rate of the forward and reverse reaction is constant in the region f - g. v. the reaction reaches equilibrium at point e as all concentrations are equal at this point. iv only i, iii and iv ii and iv ii, iv and v ii only

Explanation:

Step1: Analyze the concentration changes

In the reaction \(X + 3Y
ightleftharpoons2Z\), reactants (\(X\) and \(Y\)) are consumed and products (\(Z\)) are formed. Reactant concentrations decrease over time. Since \(Y\) has a stoichiometric coefficient of \(3\) (higher than \(X\)'s \(1\)), \(Y\) is consumed faster. So \(A\) is \(Y\), \(C\) is \(X\).

Step2: Check equilibrium regions

Equilibrium is when concentrations are constant. Region \(F - G\) shows constant concentrations (equilibrium). In equilibrium, \(v_{forward}=v_{reverse}\) (constant). Region \(E - F\) has changing concentrations (not equilibrium). At point \(E\), concentrations are equal but still changing (not equilibrium).

Answer:

II and IV