1. According to the collision theory of chemical reactions:
A. High energy collisions result in few successful reactions as there isn’t sufficient time for the products to react.
B. High energy collisions lead to the successful formation of products.
C. Low energy collisions do not occur in the gas phase.
D. Low energy collisions result in many successful reactions are there is sufficient time for the reactants to form products.
E. All of the above
2. Given N2(g) ⇋ 2 NH3(g), which scenario will allow you to eventually reach an equilibrium mixture involving these chemicals?
A. Place only H2 into a sealed vessel
B. Place only NH3 into a sealed
C. Place only N2 into a sealed vessel.
D. All of the above Scenarios
E. None of the above
3. What must be TRUE for reaction possessing a large equilibrium constant?
A. The reaction rate is slow
B. The forward reaction is favored.
C. The reverse reaction is favored.
D. The reaction rate is fast.
E. None of the above.
4. Consider the reaction: 2N2O(g) ⇋ O2(g)+2N2(g). Which of the following will cause a shift in the equilibrium to the right?
1. Add more N2O
2. Remove O2
3. Remove N2
A. 1 and 3 only
B. 2 and 3 only
C. 1 and 2 only
D. All of 1,2, and 3
E. Neither 1,2, or 3
5. If an equilibrium reaction shifts to the right when the system is cooled, this indicated that the reaction is endothermic.
A. True
B. False
6. Which of the following is a triprotic acid?
A. NH3
B. Al(OH)3
C. H3PO4
D. HNO3
E. CH3COOH
1. According to the collision theory of chemical reactions, the correct answer is A. High energy collisions result in few successful reactions as there isn't sufficient time for the products to react.
2. To eventually reach an equilibrium mixture involving N2(g) ⇋ 2 NH3(g), you would need to place only N2 into a sealed vessel. Therefore, the correct answer is C.
3. For a reaction to possess a large equilibrium constant, the forward reaction must be favored. Therefore, the correct answer is B.
4. To shift the equilibrium to the right in the reaction 2N2O(g) ⇋ O2(g)+2N2(g), you would need to add more N2O. Therefore, the correct answer is A. 1 and 3 only.
5. If an equilibrium reaction shifts to the right when the system is cooled, it indicates that the reaction is exothermic, not endothermic. Therefore, the statement is false. The correct answer is B.
6. A triprotic acid is an acid that can donate three protons (H+ ions). Among the given options, H3PO4 (phosphoric acid) is a triprotic acid. Therefore, the correct answer is C.
1. According to the collision theory of chemical reactions, the correct answer is B. High energy collisions lead to the successful formation of products. To understand why, you need to know that the collision theory states that for a reaction to occur, the reacting particles must collide with sufficient energy and correct orientation. High energy collisions provide enough energy for the bonds to break and the reaction to proceed, resulting in the successful formation of products.
2. Given the reaction N2(g) ⇋ 2 NH3(g), the scenario that will eventually reach an equilibrium mixture involving these chemicals is C. Place only N2 into a sealed vessel. This is because according to Le Chatelier's principle, the system will respond to a change in concentration by shifting the equilibrium in the opposite direction to reduce the effect of the change. Therefore, adding more N2 will cause the equilibrium to shift towards the formation of NH3 until an equilibrium mixture is reached.
3. For a reaction possessing a large equilibrium constant, the correct answer is B. The forward reaction is favored. The equilibrium constant (K) measures the ratio of products to reactants at equilibrium. A large K value indicates that the concentration of products is much greater than the concentration of reactants at equilibrium, which means the forward reaction is favored.
4. For the reaction 2N2O(g) ⇋ O2(g) + 2N2(g), the conditions that will cause a shift in the equilibrium to the right are 1. Add more N2O and 2. Remove O2. Therefore, the correct answer is C. 1 and 2 only. According to Le Chatelier's principle, adding more N2O or removing O2 will disturb the equilibrium and cause the reaction to shift in the direction that consumes the added substance or replenishes the removed substance, which in this case is towards the formation of more products.
5. If an equilibrium reaction shifts to the right when the system is cooled, this indicates that the reaction is endothermic. The correct answer is A. True. According to Le Chatelier's principle, cooling the system is equivalent to removing heat from the reaction. To counteract this decrease in temperature, the equilibrium will shift in the direction that produces more heat, which in an endothermic reaction is towards the right.
6. A triprotic acid is an acid that can donate three protons (H+ ions) per molecule. The correct answer is C. H3PO4, which is phosphoric acid, is a triprotic acid. In contrast, the other options listed (NH3, Al(OH)3, HNO3, CH3COOH) are either bases or monoprotic acids (they can only donate one proton per molecule).