Q. In a system of two blocks connected by a spring, if the spring is compressed, what is the condition for equilibrium?
A.
Net force acting on the system is zero
B.
Net momentum of the system is constant
C.
Kinetic energy is maximized
D.
Potential energy is minimized
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Solution
For equilibrium, the net force acting on the system must be zero.
Correct Answer: A — Net force acting on the system is zero
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Q. In a system where two forces act at an angle of 90 degrees, how do you find the resultant force?
A.
By adding the forces algebraically
B.
Using the Pythagorean theorem
C.
By taking the average of the two forces
D.
By subtracting the smaller force from the larger force
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Solution
The resultant force can be found using the Pythagorean theorem since the forces are perpendicular.
Correct Answer: B — Using the Pythagorean theorem
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Q. In the equilibrium constant expression Kc, what is the unit for Kc if the reaction is A(g) + B(g) ⇌ C(g)?
A.
mol/L
B.
L/mol
C.
dimensionless
D.
mol^2/L^2
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Solution
The equilibrium constant Kc is dimensionless because it is a ratio of concentrations raised to their stoichiometric coefficients.
Correct Answer: C — dimensionless
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Q. In the equilibrium reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), if SO2 is added, what will be the effect on the equilibrium?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Increase in pressure
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Solution
Adding SO2 will shift the equilibrium to the right to produce more SO3, according to Le Chatelier's principle.
Correct Answer: A — Shift to the right
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Q. In the equilibrium reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if SO3 is removed?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Increase in pressure
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Solution
Removing SO3 will shift the equilibrium to the right to produce more SO3.
Correct Answer: A — Shift to the right
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Q. In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if SO2 is removed from the system?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Increase in temperature
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Solution
Removing SO2 will shift the equilibrium to the left to produce more SO2, according to Le Chatelier's principle.
Correct Answer: B — Shift to the left
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Q. In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens to the equilibrium if the volume of the container is decreased?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Increase the rate of reaction
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Solution
Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas, which is the right side (2 moles of SO3).
Correct Answer: A — Shift to the right
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Q. In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of increasing the concentration of SO2?
A.
Shifts to the right
B.
Shifts to the left
C.
No effect
D.
Increases the rate of reaction
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Solution
Increasing the concentration of a reactant shifts the equilibrium position to the right, favoring the formation of products (SO3).
Correct Answer: A — Shifts to the right
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Q. In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of increasing the pressure on the equilibrium?
A.
Shift to the left
B.
Shift to the right
C.
No effect
D.
Depends on the temperature
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Solution
Increasing the pressure will shift the equilibrium towards the side with fewer moles of gas, which is the right side in this case (2 moles of SO3).
Correct Answer: B — Shift to the right
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Q. In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if SO3 is removed from the system?
A.
Equilibrium shifts to the left
B.
Equilibrium shifts to the right
C.
No change
D.
Equilibrium constant increases
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Solution
Removing SO3 will shift the equilibrium to the right to produce more SO3, according to Le Chatelier's principle.
Correct Answer: B — Equilibrium shifts to the right
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Q. In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the pressure is increased, which direction will the equilibrium shift?
A.
To the left
B.
To the right
C.
No shift
D.
Depends on temperature
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Solution
Increasing pressure shifts the equilibrium towards the side with fewer moles of gas, which is the right side in this case.
Correct Answer: B — To the right
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Q. In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the temperature is decreased, what will happen to the equilibrium?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Increase in pressure
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Solution
Decreasing the temperature for an exothermic reaction will shift the equilibrium to the right, favoring the formation of CH3OH.
Correct Answer: A — Shift to the right
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Q. In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if H2 is removed from the system at equilibrium?
A.
Equilibrium shifts to the right
B.
Equilibrium shifts to the left
C.
No change
D.
Equilibrium constant increases
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Solution
Removing H2 will shift the equilibrium to the left to produce more H2, thus favoring the reactants.
Correct Answer: B — Equilibrium shifts to the left
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Q. In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if H2 is removed from the system?
A.
Shift to the left
B.
Shift to the right
C.
No change
D.
Increase the rate of reaction
Show solution
Solution
Removing H2 will shift the equilibrium to the left to produce more H2, according to Le Chatelier's principle.
Correct Answer: A — Shift to the left
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Q. In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if H2 is removed?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Equilibrium constant increases
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Solution
Removing H2 will shift the equilibrium to the left to produce more H2, according to Le Chatelier's principle.
Correct Answer: B — Shift to the left
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Q. In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the volume of the container is decreased?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Increase in temperature
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Solution
Decreasing the volume increases the pressure, which shifts the equilibrium to the side with fewer moles of gas, favoring the production of CH3OH.
Correct Answer: A — Shift to the right
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Q. In the reaction: 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen to the equilibrium?
A.
Shift to the left
B.
Shift to the right
C.
No change
D.
Depends on temperature
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Solution
Decreasing the volume increases the pressure, and the equilibrium will shift to the side with fewer moles of gas, which is the left side in this case.
Correct Answer: A — Shift to the left
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Q. In the reaction: 2A(g) ⇌ B(g) + C(g), if the volume of the container is decreased, what will happen?
A.
Shift to the left
B.
Shift to the right
C.
No change
D.
Depends on the temperature
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Solution
Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas, which is the left side in this case.
Correct Answer: A — Shift to the left
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Q. In the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if the temperature is increased?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Increase in Kp
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Solution
If the reaction is exothermic, increasing the temperature will shift the equilibrium to the left, favoring the reactants.
Correct Answer: B — Shift to the left
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Q. What happens to the equilibrium constant if the reaction is reversed?
A.
K remains the same
B.
K is doubled
C.
K is inverted
D.
K is halved
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Solution
When a reaction is reversed, the equilibrium constant for the reverse reaction is the reciprocal of the equilibrium constant for the forward reaction.
Correct Answer: C — K is inverted
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Q. What happens to the equilibrium constant when a reaction is reversed?
A.
It remains the same
B.
It doubles
C.
It is inverted
D.
It is halved
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Solution
When a reaction is reversed, the equilibrium constant is inverted (1/K).
Correct Answer: C — It is inverted
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Q. What is the concentration of H+ ions in a solution with a pH of 3?
A.
0.001 M
B.
0.01 M
C.
0.1 M
D.
1 M
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Solution
[H+] = 10^(-pH) = 10^(-3) = 0.001 M
Correct Answer: A — 0.001 M
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Q. What is the effect of a catalyst on the equilibrium constant of a reaction?
A.
Increases the constant
B.
Decreases the constant
C.
No effect on the constant
D.
Depends on the reaction
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Solution
A catalyst does not affect the equilibrium constant; it only speeds up the rate at which equilibrium is reached.
Correct Answer: C — No effect on the constant
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Q. What is the effect of adding a catalyst to a chemical equilibrium?
A.
Increases the yield of products
B.
Increases the rate of reaction
C.
Shifts the equilibrium position
D.
Has no effect on the equilibrium
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Solution
A catalyst speeds up the rate of both the forward and reverse reactions equally, thus having no effect on the position of equilibrium.
Correct Answer: D — Has no effect on the equilibrium
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Q. What is the effect of adding a catalyst to a system at equilibrium?
A.
Increases the rate of the forward reaction only
B.
Increases the rate of the reverse reaction only
C.
Increases the rate of both forward and reverse reactions
D.
Shifts the equilibrium position
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Solution
A catalyst increases the rate of both the forward and reverse reactions equally, thus it does not shift the position of equilibrium.
Correct Answer: C — Increases the rate of both forward and reverse reactions
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Q. What is the effect of adding a common ion to a saturated solution?
A.
Increases solubility
B.
Decreases solubility
C.
No effect on solubility
D.
Changes the pH
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Solution
Adding a common ion decreases the solubility of a salt in a saturated solution due to the common ion effect.
Correct Answer: B — Decreases solubility
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Q. What is the effect of adding a strong acid to a buffer solution?
A.
pH increases
B.
pH decreases significantly
C.
pH remains relatively constant
D.
pH becomes neutral
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Solution
A buffer solution is designed to resist changes in pH, so adding a strong acid will cause only a small change in pH.
Correct Answer: C — pH remains relatively constant
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Q. What is the effect of adding a strong base to a buffer solution?
A.
pH decreases
B.
pH increases
C.
pH remains constant
D.
Buffer capacity increases
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Solution
Adding a strong base to a buffer solution will increase the pH, but the buffer will resist significant changes in pH due to the presence of the weak acid.
Correct Answer: B — pH increases
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Q. What is the effect of adding an inert gas at constant volume on the equilibrium of a reaction?
A.
Shifts the equilibrium to the right
B.
Shifts the equilibrium to the left
C.
No effect on the equilibrium position
D.
Increases the equilibrium constant
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Solution
Adding an inert gas at constant volume does not change the partial pressures of the reactants and products, thus it has no effect on the equilibrium position.
Correct Answer: C — No effect on the equilibrium position
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Q. What is the effect of adding an inert gas at constant volume on the equilibrium of the reaction A(g) ⇌ B(g)?
A.
Shifts to the right
B.
Shifts to the left
C.
No effect
D.
Increases the rate of reaction
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Solution
Adding an inert gas at constant volume does not change the partial pressures of the reactants or products, hence no effect on equilibrium.
Correct Answer: C — No effect
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