1 : Predict which components of the atmosphere react in the presence of lighting.
1 : N2 and H2O
2 : O2 and H2O
3 : CO2 and O2
4 : N2 and O2
2 : What will happen if the rates of forward and reverse reactions are very high?
1 : The equilibrium point will reach very soon
2 : The equilibrium point will reach very late
3 : The reaction will not attend the state of dynamic equilibrium
4 : The reaction will be practically irreversible
3 : Why the gas starts coming out when you open a can of fizzy drink?
1 : Because the solubility of the gas increases
2 : Because the gas is insoluble in water
3 : Because the gas is dissolved under pressure hands it comes out when pressure is decrease
4 : Because the solubility of the gas decrease at high pressure
4 : When a reaction will become a reversible one?
1 : If the activation energy of the forward reaction is comparable to that of backward reaction
2 : If the activation energy of the forward reaction is higher than that of the backward reaction
3 : If the activation energy of the forward reaction is lower than that of backward reaction
4 : If the enthalpy change of both the reaction is zero
5 : What will happen to the concentration of the products if a reversible reaction at equilibrium is not distribute?
1 : They will remain constant
2 : They will keep on increasing
3 : They will keep on decreasing
4 : They will remain constant for some time and then start decreasing
6 : Is reversible reaction useful for preparing compounds on a large scale?
1 : No
2 : Yes
3 : They are useful only when equilibrium lies far to the right side
4 : They are useful only when equilibrium lies far to the left side
7 : What condition should be met for the reversible reaction to achieve the state of equilibrium?
1 : All the reactants should be converted into the products
2 : 50% of the reactants should be converted into products
3 : The concentration of all the reactants and the products should become constant
4 : One on the products should be removed from the reactions mixture
8 : An inorganic chemist place one mall of PCI 5 in a container A and one mole of each CI2 and PCI3 in container B. Both the containers were sealed and heat it to the same temperature to reach the state of equilibrium. Guess about the composition of mixture in both the containers.
1 : Both the containers will have the same composition of mixtures
2 : Containers A will have more concentration of PCI3 then B
3 : Containers A will have less concentration of PCI3 then B
4 : Both the containers will have zero concentration of its reactants
9 : CaO or lime is used extensively in steel , glass and paper industries. It is produced in an exothermic reversible reaction by the decomposition of lime (CaCO3). Choose the condition to produce maximum amount of lime.
1 : Eating at high temperature in a closed vessel
2 : Hitting at high temperature in an open vessel
3 : Cooling it in a closed vessel
4 : Calling it in an open vessel
10 : What happens at equilibrium in a reversible chemical reaction?
1 : The concentrations of reactants and products remain constant
2 : The reactants are completely consumed
3 : The products decompose to form reactants only
4 : The forward reaction stops
11 : In an endothermic reaction, decreasing temperature causes:
1 : shift toward products
2 : A shift toward reactants
3 : An increase in the equilibrium constant
4 : The reaction rate to increase
12 : What is meant by chemical equilibrium?
1 : Reactants are completely converted into products
2 : The rates of the forward and reverse reactions are equal
3 : No reactions are happening
4 : All the reactants are used up
13 : for the reaction H2 +I2 →← 2HI
1 : shift equilibrium towards reactants
2 : Shift equilibrium towards products
3 : Stop reaction
4 : Have no effect on equilibrium as the number of gas molecules is the same on both sides
14 : When pressure is increased in a reaction involving gases, equilibrium shifts to:
1 : The side with more gas molecules
2 : The side with fewer gas molecules
3 : The side with equal gas molecules
4 : The reaction rate stops
15 : For the reaction 2SO2(g) + O2(g) →← 2SO3(g) ΔH = -98 kJ/mol (exothermic). How does increasing temperature affect equilibrium, If the reaction is exothermic?
1 : Equilibrium shifts toward products
2 : Equilibrium shifts toward reactants
3 : No change in equilibrium
4 : Reaction rate decreases
16 : What is the condition for an object to be in rotational equilibrium?
1 : The object must be at rest
2 : The sum of torques acting on the object must be zero
3 : The forces must be unbalanced
4 : The object must rotate at constant speed
17 : What is the effect of increasing pressure in a reaction where there are more gas molecules on the product side?
1 : Equilibrium shifts toward products
2 : Equilibrium shifts toward reactants
3 : Reaction rate decreases
4 : No effect on equilibrium
18 : Which statement is true for equilibrium in a closed system when temperature increases?
1 : The equilibrium constant changes
2 : Pressure changes automatically
3 : Concentrations of products remain constant
4 : Reaction stops
19 : What happens to the equilibrium constant when pressure changes?
1 : It increases with pressure
2 : Shifts equilibrium toward products
3 : It remains constant regardless of pressure changes
4 : Stops the reaction
20 : Which of the following is an example of static equilibrium?
1 : A book lying on a table
2 : A car moving at constant velocity
3 : A ball thrown into the air
4 : A chemical reaction in progress
21 : What is the effect of decreasing pressure on the reaction N2(g) + 3H2(g) →←2NH3(g)
1 : Shifts equilibrium toward reactants
2 : shift equilibrium towards product
3 : No effect on equilibrium
4 : stop the reaction
22 : In which type of equilibrium are both reactants and products present in the system?
1 : Static equilibrium
2 : Dynamic equilibrium
3 : Gravitational equilibrium
4 : Thermal equilibrium
23 : In which type of equilibrium do the products have more potential energy than the reactants?
1 : Unstable equilibrium
2 : Stable equilibrium
3 : Dynamic equilibrium
4 : Neutral equilibrium
24 : What effect does decreasing temperature have on the equilibrium of an endothermic reaction?
1 : A Shifts toward products
2 : Shifts toward reactants
3 : C Decreases the equilibrium constant
4 : Increases the equilibrium constant
25 : What happens to the equilibrium constant (K) when temperature is increased for an exothermic reaction?
1 : A Increases
2 : Decreases
3 : C Remains constant
4 : Depends on pressure
26 : In the reaction N2 + 3H2 →← 2NH3 increasing pressure will:
1 : A Shift equilibrium toward reactants
2 : Shift equilibrium toward products
3 : Have no effect
4 : D Favor both forward and reverse reactions equally
27 : In stable equilibrium, what happens when the object is displaced?
1 : It returns to its original position
2 : It moves farther away from the original position
3 : It remains in the new position
4 : It accelerates indefinitely
28 : What is the effect of decreasing pressure on the equilibrium of a gaseous reaction?
1 : Shirts toward the side with fewer gas molecules
2 : Shifts toward the side with more gas molecules
3 : Stops the reaction
4 : Equilibrium remains unaffected.
29 : What happens to the equilibrium position when the temperature of an exothermic reaction is increased?
1 : Shifts toward reactants
2 : Shifts toward product
3 : Remains unchanged
4 : reaction stop
30 : In a reaction where the number of gas molecules is the same on both sides, changing pressure will:
1 : Shift equilibrium toward reactants
2 : Equilibrium shifts toward products
3 : C Stop the reaction
4 : Have no effect an equilibrium position
31 : Which of the following is a characteristic of equilibrium in a reversible reaction.
1 : The system only proceeds in one direction
2 : The rate of the forward reaction is equal to the rate of the reverse reaction
3 : The system is completely static
4 : Only products are formed
32 : How does increasing pressure affect the equilibrium in a reaction with more gas molecules on the reactant side?
1 : A Shifts toward products
2 : Shifts toward reactants
3 : No effect
4 : Reaction rate decreases
33 : What is the effect of a catalyst on equilibrium?
1 : It shifts the equilibrium toward products
2 : It speeds up the attainment of equilibrium without shifting the equilibrium position.
3 : It stops the reaction from reaching equilibrium
