Answer to Question #172287 in General Chemistry for 09-j09

Question

Hydrogen gas (colorless) reacts with pure iodine vapor (purple) to give hydrogen iodide gas (colorless).

1. Write a balanced equation for this reaction: H2 (g)+ I2 (g) → 2HI (g)
2. If the equilibrium mixture of these three gases is light purple in color, what change in color would you expect to observe if more hydrogen gas were added to the system? Explain Clearly
3. If the equilibrium mixture of these three gases is light purple in color, what change in color would you expect to observe if some of the hydrogen iodide gas were removed from the system? Explain clearly.
4. Consider the following equilibrium: Heat + CaCO3 (s)  CaO (s) + CO2 (g)
5. If the pressure of CO2 (g) increases, in which direction will the equilibrium shift?Explain Clearly
6. If the temperature is increased, in which direction will the equilibrium shift? Explain Clearly

If the temperature is decreased, in which direction will the equilibrium shift? Explain Clearly

Answer 1

1.H2 (g)+ I2 (g) → 2HI (g)

2.When the concentration of one of the starting substances increases, the equilibrium shifts in the direction of the formation of reaction products. Color change from light purple to colorless

3.Reducing the concentration of the starting substance will start the reaction on the reverse path. the color will be even less light purple

4.CaCO3 (s)+Q= CaO (s) + CO2 (g)

5.When the pressure increases, the chemical equilibrium shifts towards the reaction, accompanied by a decrease in the total number of gases

6.Increase the temperature, therefore, the equilibrium will shift towards -Q, to the right

As the temperature increases, the equilibrium shifts towards the endothermic reaction, and as the temperature decreases, it shifts towards the exothermic reaction.