Initially, a container contains only H 2 and I 2 gas molecules (H2 + I2 --> <--
ID: 633923 • Letter: I
Question
- Initially, a container contains only H2 and I2 gas molecules (H2 + I2 --> <-- 2HI(g). Describe the movement of the molecules and consider whether or not they interact. What will you see as the molecules react?
- Assume that equilibrium is achieved within 15 minutes. Describe what you will see once the reaction has achieved equilibrium. Can you tell from the information given whether there will be more reactants or more products at equilibrium?
- What will you see 20 minutes after the reaction has achieved equilibrium? Will this situation be different from what you will see 2 minutes after the reaction has achieved equilibrium?
- imagine that all of the gas is evacuated so that the container is completely empty of gas molecules. Then the container is refilled with HI molecules only. What will happen when the HI molecules collide with each other? Will they react, even though they are products of the first reaction?
- Describe what you will see after equilibrium has been established in this second system.
- Finally, compare the first scenario with the second scenario. What similarities or differences will you find after both systems have reached equilibrium? (Assume that there is the same number of molecules present in both scenarios.)
Explanation / Answer
1)
they interact and forms HI molecule and establishes equillibrium..we see as the molecules reacted the pressure of the vessel is reduced due to formation of one compound
2)
we cannot tell which is more either of reactant or products..it completely depends on the equillibrium constant for that reaction .. complete process can be decided by equillibrium constan
3)
no change in the concerntration of the molecules once the it recheade the equillibrium