H2(g) + I2(g) 2 HI(g)
The forward reaction above is exothermic. At equilibrium, what happens if I2 is removed from the reaction mixture at constant temperature and volume?
The reaction absorbs energy.
The reaction releases energy.
[H2] increases.
[H2] decreases.
[H2] remains constant.
[HI] increases.
[HI] decreases.
[HI] remains constant.
i tried releases energy, H2 decreases, and HI increases.
You didn't place an arrow. If the reaction is
H2 + I2 ==> 2HI + heat and you remove I2, the reaction will shift to the left. That means,
a. (H2) increases.
b. (I2) decreases.
c. (HI) decreases.
d. heat is absorbed.
sdad
When I2 is removed from the reaction mixture at constant temperature and volume, according to Le Chatelier's principle, the equilibrium will shift in a direction that opposes the change. Since I2 is a reactant in the forward reaction, its removal will cause the reaction to shift towards the left to replace the lost I2. As a result, [H2], which is a reactant, will decrease, and [HI], which is a product, will also decrease. Therefore, the correct statements in this scenario are:
1. The reaction releases energy.
2. [H2] decreases.
3. [HI] decreases.
To determine what happens to the system when I2 is removed from the reaction mixture at constant temperature and volume, we need to consider the Le Chatelier's principle.
First, let's understand the reaction. The given equation represents the synthesis of hydrogen iodide (HI) from hydrogen gas (H2) and iodine gas (I2). The balanced equation shows that two moles of HI are formed from one mole of H2 and one mole of I2.
Since the forward reaction is exothermic, it releases energy. This means that heat is a product of the reaction. Now, when I2 is removed from the reaction mixture, the equilibrium shifts to compensate for the change and tries to replace the removed I2.
According to Le Chatelier's principle, if a reactant is removed from a system, the equilibrium shifts in the forward direction to counteract the change. In other words, the system will try to replenish the I2 that was removed.
As a result, the equilibrium would shift to the right, favoring the forward reaction. This means that more HI would be produced to compensate for the loss of I2. Since H2 is one of the reactants, a decrease in I2 would cause H2 to also decrease because it is being consumed in the reaction to form more HI.
Therefore, the correct answers would be:
- The reaction releases energy.
- [H2] decreases.
- [HI] increases.
It's important to note that the concentration of H2 would decrease, but it does not necessarily mean that the concentration of H2 gas actually decreases. The decrease refers to a shift in equilibrium, causing a decrease in the concentration relative to the new equilibrium position.