Study the following equation.
Fe(s) + 2 HCl(aq) → H2(g) + FeCl2(aq)
What happens to the iron metal when it is reacted in a closed container to produce hydrogen gas in this manner?
Select all that apply.
The rate of the reverse reaction increases as hydrogen gas accumulates. (correct)
The rate of the forward reaction is at its maximum when the reaction first starts.
The rate of the reverse reaction decreases as pressure from the hydrogen gas accumulates.
Oh, iron in a closed container? That's one way to keep it from rusting! Now, let's see what happens.
First off, when the reaction starts, the forward reaction will be rocking and rolling at its maximum rate. It's like a sprinter at the start of the race, full of energy and ready to go.
As time goes on, hydrogen gas starts to accumulate. And because the reverse reaction involves the formation of hydrogen gas, it's going to get more tempting for it to kick in. Just imagine a party where everyone gathers around the snack table – the reverse reaction starts to get a bit more active as the pressure from the hydrogen gas builds up.
But hey, it's not all bad news for the iron! As the reverse reaction kicks in, it actually helps slow down the rate of the forward reaction. It's like a self-regulating system. The iron is going, "Hold on, hold on, let's not rush into things," while the hydrogen gas is saying, "Come on, guys, let's party!"
So, to sum it up, the rate of the reverse reaction increases as hydrogen gas accumulates, but the rate of the forward reaction decreases as pressure from the hydrogen gas builds up.
The correct statements are:
- The rate of the reverse reaction increases as hydrogen gas accumulates.
- The rate of the forward reaction is at its maximum when the reaction first starts.
To determine what happens to the iron metal when it reacts with hydrochloric acid (HCl) to produce hydrogen gas, we need to analyze the given chemical equation:
Fe(s) + 2 HCl(aq) → H2(g) + FeCl2(aq)
Here's how we can understand what happens to the iron metal in this reaction:
1. The rate of the reverse reaction increases as hydrogen gas accumulates (Correct): In this reaction, iron (Fe) reacts with hydrochloric acid (HCl) to produce hydrogen gas (H2) and iron chloride (FeCl2). As hydrogen gas accumulates in the closed container, the concentration of hydrogen molecules increases. According to Le Chatelier's principle, an increase in the concentration of one of the reactants or products in a system will shift the equilibrium towards the opposite direction. In this case, the increase in hydrogen gas concentration will favor the reverse reaction, which involves the recombination of hydrogen gas with iron chloride to reform iron metal. Therefore, the rate of the reverse reaction increases as hydrogen gas accumulates.
2. The rate of the forward reaction is at its maximum when the reaction first starts (Incorrect): The rate of the forward reaction refers to the rate at which reactants are converted into products. At the beginning of the reaction, when the reactants are first mixed, the concentration of reactants is at its highest. This results in a rapid reaction rate, but it is not necessarily at its maximum. The rate of the forward reaction typically decreases over time as the reactants are consumed, and the concentration of reactants decreases.
3. The rate of the reverse reaction decreases as pressure from the hydrogen gas accumulates (Incorrect): The rate of the reverse reaction is dependent on the concentration of reactants and products, rather than the pressure in a closed container. While the pressure may increase due to the accumulation of hydrogen gas, it does not directly affect the rate of the reverse reaction. The pressure in the container is determined by the initial volume of the container, the number of moles of gas produced, and the temperature, according to the ideal gas law. However, it does not impact the rate of the reverse reaction.
In conclusion, the correct statement is: The rate of the reverse reaction increases as hydrogen gas accumulates.