1. Which one of the following would make the most suitable catalyst in the decomposition of hydrogen peroxide (H2O2)?
A. Carbon dioxide (CO2)
B. Sodium chloride (NaCl)
C. Magnesium oxide (MgO)
D. Manganese dioxide (MnO2)
2. If the temperature of a reaction is decreased, what effect will this have on the rate of reaction?
A. It will have no effect.
B. The reaction will stop.
C. The rate of reaction will increase.
D. The rate of reaction will decrease.
3. Given the equilibrium reaction in a closed system. What will be the result of an increase in temperature?
H2(g) + I2(g) + heat → 2 HI(g).
A. The equilibrium will shift to the left and [H2] will increase.
B. The equilibrium will shift to the left and [H2] will decrease.
C. The equilibrium will …show more content…
The equilibrium will shift to the right and [HI] will decrease.
4. 20 grams of magnesium were placed in a conical flask. Which one of the following solutions, if added, would produce 100 mL of hydrogen gas the fastest?
A. 100 mL of 4 M sulfuric acid
B. 200 mL of 2 M sulfuric acid
C. 400 mL of 1 M sulfuric acid
D. 50 mL of 8 M sulfuric acid
5. Why does the rate of reaction increase when powdered calcium carbonate is used instead of marble chips?
A. The powdered calcium carbonate acts as a catalyst.
B. There is an increase of the particle size of the calcium carbonate.
C. There is an increase of the surface area of the calcium carbonate.
D. There is an increase of the concentration of the calcium carbonate.
6. Which of the following reactions will start with the highest rate?
A. 5 g of limestone chips in 100 mL of 0.1 M HCl at 25ºC.
B. 5 g of limestone chips in 100 mL of 0.1 M HCl at 45ºC.
C. 5 g of limestone powder in 100 mL of 0.1 M HCl at 25ºC.
D. 5 g of limestone powder in 100 mL of 0.1 M HCl at 45ºC.
7. What effect does doubling the concentration of one of the reactants have on the rate of reaction?
A. It has no effect.
B. The rate of reaction s halved.
C. It increases the rate of reaction.
D. It decreases the rate of
A. Carbon dioxide (CO2)
B. Sodium chloride (NaCl)
C. Magnesium oxide (MgO)
D. Manganese dioxide (MnO2)
2. If the temperature of a reaction is decreased, what effect will this have on the rate of reaction?
A. It will have no effect.
B. The reaction will stop.
C. The rate of reaction will increase.
D. The rate of reaction will decrease.
3. Given the equilibrium reaction in a closed system. What will be the result of an increase in temperature?
H2(g) + I2(g) + heat → 2 HI(g).
A. The equilibrium will shift to the left and [H2] will increase.
B. The equilibrium will shift to the left and [H2] will decrease.
C. The equilibrium will …show more content…
The equilibrium will shift to the right and [HI] will decrease.
4. 20 grams of magnesium were placed in a conical flask. Which one of the following solutions, if added, would produce 100 mL of hydrogen gas the fastest?
A. 100 mL of 4 M sulfuric acid
B. 200 mL of 2 M sulfuric acid
C. 400 mL of 1 M sulfuric acid
D. 50 mL of 8 M sulfuric acid
5. Why does the rate of reaction increase when powdered calcium carbonate is used instead of marble chips?
A. The powdered calcium carbonate acts as a catalyst.
B. There is an increase of the particle size of the calcium carbonate.
C. There is an increase of the surface area of the calcium carbonate.
D. There is an increase of the concentration of the calcium carbonate.
6. Which of the following reactions will start with the highest rate?
A. 5 g of limestone chips in 100 mL of 0.1 M HCl at 25ºC.
B. 5 g of limestone chips in 100 mL of 0.1 M HCl at 45ºC.
C. 5 g of limestone powder in 100 mL of 0.1 M HCl at 25ºC.
D. 5 g of limestone powder in 100 mL of 0.1 M HCl at 45ºC.
7. What effect does doubling the concentration of one of the reactants have on the rate of reaction?
A. It has no effect.
B. The rate of reaction s halved.
C. It increases the rate of reaction.
D. It decreases the rate of