AP MCQ 05ABCDEFGHIJK PART 2 Question 01: Which situation best describes a successful collision (one that leads to a chemical reaction)? The reactants collide The reactants collide with sufficient energy The reactants collide with sufficient energy and the correct orientation All collisions are successful Question 02: Collision theory predicts which of the following? That all reactions are bimolecular That collision geometry (orientation) is irrelevant in chemical reactions That more successful collisions will occur with increasing activation energy That a reaction will not occur if the collision occurs with energy that is less than the activation energy Question 03: Which of the following is a bimolecular reaction? A + A → B A → B 2A + B → C A + 2B → C + D Question 04: The rate of a chemical reaction will increase with An increasing number of collisions with sufficient energy and correct orientation Increasing activation energy Increasing molecularity Increasing number of elementary steps Question 05: Reaction rate decreases if the frequency of collisions Increases Is held constant Reaches equilibrium Decreases Question 06: Why is the reaction below, unlikely to take place in a single, elementary step? A + 2B + C → Products Too much energy is required for a single step reaction It is unlikely that A will ever collide with C since B is between A and C B has to be split into two separate pieces before a reaction can take place, and this must happen in one step, and the remainder of the reaction in other steps The collision of four particles, with the correct collision geometry and orientation, is statistically highly unlikely Question 07: Consider the reaction shown below that takes place in two, elementary steps that make up a more complex, overal reaction. Step 1: O3(g) + HO(g) → HO2(g) + O2(g) Step 2: HO2(g) + O(g) → HO(g) + O2(g) What is the molecurality of the second step? unimolecular bimolecular trimolecular higher than trimolecular Question 08: In a reaction where a very large proportion of the molecules involved have energies that are equal to or greater than the activation energy, it is observed that the reaction is still relatively slow. What is the most reasonable explanation for this? The molecules are not colliding with one another The molecules are colliding, but the collision geometry is incorrect The activation energy is too low to induce a reaction The molecules are moving so fast that they 'bounce' off one another before reacting Question 09: What is the molecularity of the elementary reaction shown below? 2HI → H2 + I2 0 1 2 4 Question 10: Which of the following will be found at the highest energy on a reaction enthalpy profile? The products The reactants The transition state The intermediate Δ