In a chemical reaction, the forward rate is greater than the reverse rate. Which statement about the reaction is correct?
The reaction is reversible.
The reaction will continue until the reactant is used up.
The concentrations of the reactant and the product are equal.
The reaction is at dynamic equilibrium.
1. Nitrogen and hydrogen combine at the same rate that ammonia breaks down.
2. Both calcium carbonate and sodium carbonate are being produced.
3. The reaction is reversible.
4. 300,000 km/s
5. The people are moving much slower than the speed of light so the ground acts as a frame of reference.
The correct statement about the reaction is:
"The reaction is reversible."
To determine this, we compare the rates of the forward reaction and the reverse reaction. If the forward rate is greater than the reverse rate, it means that the forward reaction is occurring at a faster rate than the reverse reaction. This implies that in the given conditions, the reaction is not proceeding solely in one direction, but rather in both the forward and reverse directions leading to a reversible reaction.
The other options are not necessarily true based on the given information. The fact that the forward rate is greater than the reverse rate does not imply that the reaction will continue until the reactant is used up. The concentrations of the reactant and product can be different depending on the stoichiometry of the reaction and the initial conditions. Finally, the information provided does not indicate whether the reaction is at dynamic equilibrium, which is a state where the rate of the forward reaction is equal to the rate of the reverse reaction, and the concentrations of reactants and products do not change over time.