Question

Q1. Name 5 factors which can affect the rate of a reaction?

Q2. Which of the following statements is false?[1] The minimum amount of energy needed for a reaction to occur is called the activation energy. [2] The rate of a reaction depends on the magnitude of the activation energy. [3] A catalyst increases the rate constant in a reaction. [4] The frequency of collisions is ultimately the only factor which affects the rate of a reaction. [5] None of the above.

Q3. Which of the following will not affect the position of a chemical equilibrium?[1] Changing the temperature[2] Adding a catalyst[3] Changing the volume[4] Changing the concentration of the products[5] None of the above

Q4. Consider the following exothermic reaction: N2 (g) + 3H2 (g) ⇆ 2NH3 (g).For this reaction, answer questions below.

a). What will happen to the reaction mixture at equilibrium if some more N2 (g) is added?
b). What will happen to the reaction mixture at equilibrium if the temperature is decreased?
c). What will happen to the reaction mixture at equilibrium if some helium gas is added?
d). What will happen to the reaction mixture at equilibrium if the volume of the container is increased?
e). What will happen to the reaction mixture at equilibrium if the pressure is increased?

Q5.Which substance can be classified as a Lewis base?[1] HCl,[2] BF3,[3] Ca2+,[4] HF, [5] NH3

Q6. Which of the following is a conjugate acid-base pair?[1] F- and NaF, [2] H2SO4 and HSO4-, [3] PH3 and PF3,[4] Br2 and Br-, [5] HCl and HClO4

Q7. Which of the following will give an acidic mixture?
[1] Mixing equal volumes of 1.0 M HCl and 1.0 M KOH
[2] Mixing 2.0 L of 1.0 M H2SO4 with 4.0 L of 1.0 M KOH
[3] Mixing equal volumes of 1.0 M KOH and water
[4] Mixing 1.0 L of 1.0 M HCl with 2.0 L of 1.0 M KOH
[5] Mixing equal volumes of 1.0 M H3PO4 and 1.0 M NaOH

Q8.Which of the following is the strongest acid?[1] HNO3, [2] HF, [3] H2S, [4] CH3COOH
[5] HPO42

Q9, Which of the following is a salt? [1] KOH, [2] HBr, [3] BF3, [4] NH3, [5] NaBr

Q10. As the hydrogen ion concentration of an aqueous solution increases, what will happen to the hydroxide ion concentration?

Answer 1

1] The temperature of the reaction, The concentration of the reactants, Surface area of reactants, Pressure (for gas reactions), Catalysts

2] none of the above

3] Adding a catalyst does not affect the position of equilibrium

4] for given reaction a) if we add some more N2, the equilibrium would shift to the right side( fewer moles of gas ) in order to use up of extra N2. b) if the temperature is decreased  the equilibrium would shift towards the side with the heat term ( produce heat) c) if some helium gas is added, the volume will increase and the equilibrium would shift to left in given equation ( higher moles) d) if the volume of the container is increased, total pressure decrease and equilibrium would shift to left e) if the pressure is increased the equilibrium would shift to the right side

5] NH3 because it can donate its lone pair of electrons

6] H2SO4 and HSO4^- because H2SO4+H2O=HSO4^- + H3O⁺

7] Mixing 1.0 L of 1.0 M HCl with 2.0 L of 1.0 M KOH gives acidic salt

8]  HNO3

9] NaBr it is formed by neutralization of NaOH + HBr

10] As the hydrogen ion concentration of aqueous solution increases, the hydroxide ion concentration will decrease.