State and explain two observations made when magnesium ribbon is lowered into a gas jar full of carbon (IV) oxide. Write a balanced chemical equation for the reaction. What does point M represent in t

Here are the solutions to the questions:

16.(a) State and explain two observations made when magnesium ribbon is lowered into a gas jar full of carbon (IV) oxide (3mk)

• Observation 1: The magnesium ribbon continues to burn with a bright white flame.
  • Explanation: Magnesium is a very reactive metal and is able to reduce carbon(IV) oxide, continuing to burn even in the absence of oxygen.
• Observation 2: A white solid (magnesium oxide) and black specks (carbon) are formed.
  • Explanation: Magnesium reacts with carbon(IV) oxide to form white magnesium oxide and black carbon.

16.(b) Write a balanced chemical equation for the reaction that took place in a) above.

$$2\text{Mg}(s) + \text{CO}_2(g) \xrightarrow{\text{heat}} 2\text{MgO}(s) + \text{C}(s)$$

17. The energy level diagram below shows the effect of a catalyst on the reaction.

17.(a) What does point M represent? (1Mk)
Point M represents the activated complex (or transition state) of the uncatalyzed reaction. The energy difference from the reactants to point M is the activation energy of the uncatalyzed reaction.