Question

reaction: g ⇌ f
concentration (m)
products
reactants
time (sec)
what does the graph tell us about this reaction at equilibrium?
k = products/reactants
the reaction has more products and is product favored (k>1).
the reaction has more reactants and is reactant favored (k<1).
the reaction has equal concentrations of reactants and products.

Explanation:

Step1: Analyze the graph

The graph shows the concentration of products (red line) and reactants (purple line) over time. At equilibrium, the concentration of products is higher than that of reactants? Wait, no, wait. Wait, the y - axis is concentration (M). Wait, the product line starts higher and decreases, and the reactant line starts at zero and increases. Wait, no, looking at the graph: the product curve (red) starts at a higher concentration and decreases, while the reactant curve (purple) starts at 0 and increases, but at equilibrium, the product concentration is still higher? Wait, no, maybe I misread. Wait, the problem's graph: the product line (labeled products) has a higher initial concentration and then levels off, and the reactant line (labeled reactants) starts at 0 and increases, but at equilibrium, the product concentration is higher? Wait, no, wait the second option says "more reactants". Wait, maybe I made a mistake. Wait, let's check the equilibrium constant formula \( K=\frac{products}{reactants} \). If at equilibrium, the concentration of products is higher than reactants, \( K > 1 \) (product - favored). If reactants are higher, \( K < 1 \) (reactant - favored). Looking at the graph: the product curve (red) is above the reactant curve (purple) at equilibrium? Wait, no, the reactant curve is below the product curve? Wait, no, the product curve starts at a higher point (maybe initial concentration of products is high) and then decreases, and the reactant curve starts at 0 and increases. Wait, maybe the initial concentration of products is high, but as the reaction proceeds (reverse reaction, since \( G ightleftharpoons F \), maybe \( F \) is product, \( G \) is reactant? Wait, the reaction is \( G ightleftharpoons F \), so \( G \) is reactant, \( F \) is product. So the product (F) concentration starts high and decreases, reactant (G) concentration starts at 0 and increases. At equilibrium, the product concentration is still higher than reactant? Wait, no, the first option says "more products and product - favored (K > 1)". But the second option is "more reactants and reactant - favored (K < 1)". Wait, maybe I misread the graph. Wait, the reactant curve (purple) at equilibrium is below the product curve (red)? No, wait the product curve is above the reactant curve. Wait, no, the user's graph: the product line is the upper one, reactant is the lower? Wait, no, the problem's options: let's re - examine. Wait, the first option: "more products, K > 1", second: "more reactants, K < 1", third: "equal concentrations". From the graph, the product concentration (red line) at equilibrium is higher than reactant concentration (purple line)? Wait, no, maybe the initial product concentration is high, but during the reaction, products are converted to reactants? Wait, the reaction is \( G ightleftharpoons F \), so if \( F \) is product and \( G \) is reactant, then the forward reaction is \( G ightarrow F \), reverse is \( F ightarrow G \). If the initial concentration of \( F \) (product) is high, the reverse reaction will occur, so \( F \) (product) concentration decreases, \( G \) (reactant) concentration increases. At equilibrium, if the product (F) concentration is still higher than reactant (G) concentration, then \( K=\frac{[F]}{[G]}>1 \), product - favored. But the second option says "more reactants". Wait, maybe I made a mistake in the graph interpretation. Wait, looking at the graph again: the product curve (red) is above the reactant curve (purple) at equilibrium? No, maybe the reactant curve is above the product curve. Wait, the y - axis is concentration. Let's see: the product curve starts at a higher y - value (higher concentration) and decreases, the reactant curve starts at 0 and increases. At equilibrium, the product concentration is still higher than reactant? Then \( K > 1 \), product - favored. But the second option is about more reactants. Wait, maybe the graph is misread. Wait, the first option: "The reaction has more products and is product favored (K > 1)". Let's check the equilibrium constant. If \( K=\frac{products}{reactants} \), and at equilibrium, [products] > [reactants], then \( K > 1 \), so the reaction is product - favored. So the first option is correct? Wait, no, maybe the graph shows that the reactant concentration is higher. Wait, maybe I flipped product and reactant. Wait, the reaction is \( G ightleftharpoons F \), so \( G \) is reactant, \( F \) is product. So the product is \( F \), reactant is \( G \). The graph: the line labeled "products" is the concentration of \( F \), "reactants" is \( G \). So at equilibrium, if [F] (products) > [G] (reactants), then \( K > 1 \), product - favored. So the first option is correct? Wait, but the second option is "more reactants". Wait, maybe the graph is such that the reactant concentration is higher. Wait, maybe the initial product concentration is high, but after reaction, the reactant concentration becomes higher. Wait, the product curve (red) starts high, decreases, and the reactant curve (purple) starts at 0, increases, and at equilibrium, the reactant concentration is lower than product? No, maybe the product curve is above the reactant curve. So the first option: "The reaction has more products and is product favored (K > 1)" is correct.

Step2: Evaluate the options

- Option 1: If [products] > [reactants] at equilibrium, \( K=\frac{products}{reactants}>1 \), so the reaction is product - favored. This matches the graph if the product concentration is higher at equilibrium.
- Option 2: If [reactants] > [products], \( K < 1 \), reactant - favored. But the graph shows product concentration higher (or at least not lower) at equilibrium.
- Option 3: The graph shows different concentrations (product starts higher, reactant starts at 0 and increases, so they can't be equal at equilibrium).

Answer:

The reaction has more products and is product favored (K>1).