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1It is the state in which both reactants and products are present in the same concentrations .
- AReversible Reactions
- BChemical Equilibrium
- CIrreversible Reactions
2The chemical reactions in which the products formed do not combine to give the reactants.
- AIrreversible Reactions
- BReversible Reactions
- CChemical Equilibrium
- DEquilibrium Constant
3The relationship between forward and reverse reactions in an equilibrium can be expressed mathematically by?
- AEquilibrium Constant
- BIrreversible Reactions
- CReversible Reactions
- DChemical Equilibrium
4 products can react to give back to the reactants and vice versa.
- AIrreversible Reactions
- BReversible Reactions
- CChemical Equilibrium
- DEquilibrium Constant
5H2(g) + I2(g) ⇌ 2HI(g) is what type of equation ?
- AIrreversible Reactions
- BReversible Reactions
6 2KClO3(s) → 2KCl(s) + 3O2(g) is what type of equation?
- AIrreversible Reactions
- Breversible Reaction
7Products are always in the numerator and reactants are always in the denominator.
- ATrue
- BFalse
8Rate of forward reaction =k2[C]m[D]n
- ATrue
- BFalse
9 Rate of forward reaction=k1[A]a[B]b
- ATrue
- BFalse
10 Rate of reverse reaction = k2[C]m[D]n
- ATrue
- BFalse
11K1/k2 =Keq is called equilibrium constant.
- ATrue
- BFalse
12.Keq<1 indicates a forward reaction.
It means the concentrations of reactants are much higher than those of the products.- ATrue
- BFalse
13the concentrations of reactants and products are same.
- AKeq<1 indicates a forward reaction.
- BKeq=1 indicates an equilibrium reaction.
- CKeq >1 indicates a reverse reaction.
14 the concentrations of the products are much greater than those of the reactants.
- AKeq >1 indicates a reverse reaction.
- BKeq<1 indicates a forward reaction.
- CKeq=1 indicates an equilibrium reaction.
15It means the concentrations of reactants are much higher than those of the products.
- AKeq >1 indicates a reverse reaction.
- B.Keq=1 indicates an equilibrium reaction.
- C.Keq<1 indicates a forward reaction.
16.Keq=1 indicates an [blank_start]equilibrium[blank_end] reaction.
- Aequilibrium
17Keq<1 indicates a [blank_start]forward[blank_end] reaction.
- Aforward
18.Keq >1 indicates a [blank_start]reverse[blank_end] reaction.
- Areverse
19Le-Chatelier's Principle ststes that When a stress (change in concentration/pressure/temp/volume) is applied to an [blank_start]equilibrium[blank_end], it will shift itself in the direction to [blank_start]nullify[blank_end] the [blank_start]stress[blank_end] applied.
- Aequilibrium
- Bnullify
- Cstress
20rate of concentration is [blank_start]change in concentration r / change in[blank_end] [blank_start]concentration of the products per unit[blank_end] time.
- Achange in concentration r / change in
- Bconcentration of the products per unit
21In the manufacture of sulphuric acid (H2SO4), sulphur trioxide is prepared, which is dissolved in water to get sulphuric acid.
- ATrue
- BFalse
22 Effect of Concentration on H2SO4.
- AIf the concentration of reactant (SO2) increases, the equilibrium is shifted to the right (forward direction).
- BIf the concentration of reactant (SO2) decreases, the equilibrium is shifted to the left (reverse direction).
23The effects of the concentration of product in H2S04
- AIf the concentration of product (SO3) increases, the equilibrium is shifted to the right (reverse direction).
- BIf the concentration of product (SO3) increases, the equilibrium is shifted to the left (reverse direction).
- CIf the concentration of product (SO3) decreases, the equilibrium is shifted to the right(forward direction).
24 Effect of Volume and Pressure on H2S04
In this reaction, 2 moles of SO2 and 1 mole of O2 reacts to give 2 moles of SO3.- AIn this reaction, 1 moles of SO2 and 1 mole of O2 reacts to give 2 moles of SO3.
- BIn this reaction, 5 moles of SO2 and 1 mole of O2 reacts to give 2 moles of SO3.
- CIn this reaction, 2 moles of SO2 and 1 mole of O2 reacts to give 2 moles of SO3.
- DIn this reaction, 3moles of SO2 and 2 mole of O2 reacts to give 2 moles of SO3.
25 Effect of Volume and Pressure on H2SO4.
- AWhen pressure of SO2 or O2 is decreased, there is decrease in the volume. Hence the equilibrium is shifted to forward direction to give more product (SO3).
- BWhen pressure of SO2 or O2 is increased, there is decrease in the volume. Hence the equilibrium is shifted to forward direction to give more product (SO3).
- CWhen pressure of SO2 or O2 is increased, there is decrease in the volume. Hence the equilibrium is shifted to reverse direction to give more product (SO3).
- DWhen pressure of SO2 or O2 is decreased, there is increase in the volume. Hence the equilibrium is shifted to forward direction to give more product (SO3).
26. Effect of Temperature on H2SO4.
- AHere -190 KJ represents it is an exothermic reaction. So increase in temp will shift the equilibrium to the reverse direction.
- BHere -190 KJ represents it is an endothermic reaction. So increase in temp will shift the equilibrium to the reverse direction.
- CHere -190 KJ represents it is an exothermic reaction. So decrease in temp will shift the equilibrium to the reverse direction.
- DHere -190 KJ represents it is an exothermic reaction. So decrease in temp will shift the equilibrium to the forward direction.
27 Optimum conditions in H2SO4
- ATo get good yield of product, the pressure of 1100-1400 mm of Hg and the temperature 420- 460°C is used in this reaction
- BTo get good yield of product, the pressure of 1200-1300 mm of Hg and the temperature 420- 450°C is used in this reaction
- CTo get good yield of product, the pressure of 1300-1400 mm of Hg and the temperature 430- 450°C is used in this reaction
- DTo get good yield of product, the pressure of 1100-1300 mm of Hg and the temperature 420- 450°C is used in this reaction
28Manufacture of Ammonia is called?
- ABirkland-Eyde Process
- BHaber process
29The manufacture of Nitric oxide is called?
- ABirkland-Eyde Process
- BHaber’s Process
30Effect of Concentration NH3.
- AIf the concentration of reactants decreases, the equilibrium is shifted to forward direction.
- BIf the concentration of reactants increases, the equilibrium is shifted to reverse direction.
- CIf the concentration of reactants increases, the equilibrium is shifted to forward direction.
31Effect of Concentration NH3.
- AIf the concentration of product increases, the equilibrium is shifted to the forward direction.
- BIf the concentration of product increases, the equilibrium is shifted to the reverse direction.
- CIf the concentration of product decreases, the equilibrium is shifted to the reverse direction.
32 Effect of Volume and Pressure ON NH3.
- AHere 4 moles of reactants gives 2 moles of products.
- BHere 3 moles of reactants gives 3 moles of products.
- CHere 2 moles of reactants gives 2 moles of products.
33 Effect of Volume and Pressure ON NH3.
- AAs an increase of pressure will cause decrease in volume.
- BAs an decrease of pressure will cause decrease in volume.
34
Effect of Volume and Pressure on NH3- ATherefore, increase in pressure will favour forward reaction
- BTherefore, increase in pressure will favour reverse reaction
35Effect of Temperature on NH3
In an exothermic reaction, increase in temperature, always shifts the equilibrium to the reverse direction.- AIn an exothermic reaction, increase in temperature, always shifts the equilibrium to the forward direction.
- BIn an exothermic reaction, decrease in temperature, always shifts the equilibrium to the reverse direction.
- CIn an exothermic reaction, increase in temperature, always shifts the equilibrium to the reverse direction.
36Effect of Temperature on NH3
- ASince ammonia formation is an exothermic reaction, high temperature will be favourable for higher yield.
- BSince ammonia formation is an endothermic reaction, low temperature will be favourable for higher yield.
- CSince ammonia formation is an exothermic reaction, low temperature will be favourable for higher yield.
37 Optimum conditions in NH3.
- AFor higher yield of ammonia, pressure of 1100 mm of Hg and temperature 420 - 450°C is used.
- BFor higher yield of ammonia, pressure of 1200 mm of Hg and temperature 420 - 460°C is used.
- CFor higher yield of ammonia, pressure of 1100 mm of Hg and temperature 440 - 450°C is used.
38Manufacture of Nitric oxide is called Birkland-Eyde Process.
- ATrue
- BFalse
39Effect of Concentration on HNO3.
- AIf the concentration of reactants decreases, the equilibrium is shifted to forward direction.
- BIf the concentration of reactants increases, the equilibrium is shifted to forward direction.
- CIf the concentration of reactants increases, the equilibrium is shifted to reverse direction.
40 Effect of Volume and Pressure on HNO3.
- AHere no change in volume i.e. n = 0, so the equilibrium is affected by any change in pressure
- BHere changes in volume occurs, so the equilibrium is not affected by any change in pressure
- CHere no change in volume i.e. n = 0, so the equilibrium is not affected by any change in pressure
41 Effect of Temperature in HNO3: It is an [blank_start]endothermic[blank_end] reaction i.e., heat is absorbed during the reaction. An [blank_start]increase[blank_end] in temperature will favour the [blank_start]forward[blank_end] reaction i.e., more nitric oxide is formed at [blank_start]higher[blank_end] temperature.
- Aendothermic
- Bexothermic
- Cincrease
- Ddecrease
- Ereverse
- Fforward
- Ghigher
- Hlower
42In blood cells: The concentration of CO2 is relatively [blank_start]high[blank_end].
- Alow
- Bmedium
- Chigh
43•In lungs:Breaking up of the carbonic acid and creating carbon dioxide, which we exhale.
- ATrue
- BFalse
44Each hemoglobin molecule attaches to four oxygen atoms. It is responsible for transporting oxygen to the cells.
- ATrue
- BFalse
45Here heam represents [blank_start]iron[blank_end] and globin represents the [blank_start]protein[blank_end] part.
- Airon
- Bprotein
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- Quiz on Untitled, created by Keresa Benjamin on 30/11/2018.
- Author
- Keresa Benjamin
- Language
- English
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