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MCQOPTIONS
This section includes 11242 Mcqs, each offering curated multiple-choice questions to sharpen your Joint Entrance Exam - Main (JEE Main) knowledge and support exam preparation. Choose a topic below to get started.
| 751. |
The hydrogen ion concentration of 0.2 N \[C{{H}_{3}}COOH\] which is 40% dissociated is |
| A. | 0.08 N |
| B. | 0.12 N |
| C. | 0.80 N |
| D. | 1.2N |
| Answer» B. 0.12 N | |
| 752. |
For the equilibrium system \[2HX(g)\rightleftharpoons {{H}_{2}}(g)+{{X}_{2}}(g)\] the equilibrium constant is \[1.0\times {{10}^{-5}}\]. What is the concentration of HX if the equilibrium concentration of \[{{H}_{2}}\] and \[{{X}_{2}}\] are\[1.2\times {{10}^{-3}}M\], and \[1.2\times {{10}^{-4}}M\] respectively. |
| A. | \[12\times {{10}^{-4}}M\] |
| B. | \[12\times {{10}^{-3}}M\] |
| C. | \[12\times {{10}^{-2}}M\] |
| D. | \[12\times {{10}^{-1}}M\] |
| Answer» D. \[12\times {{10}^{-1}}M\] | |
| 753. |
8 mol of \[A{{B}_{3}}(g)\]are introduced into a \[1.0\text{ }d{{m}^{3}}\]vessel. If it dissociates as \[2A{{B}_{3}}(g)\rightleftharpoons {{A}_{2}}(g)+3{{B}_{2}}(g)\]. At equilibrium, 2 mol of \[{{A}_{2}}\] are found to be present. The equilibrium. constant of this reaction is |
| A. | 2 |
| B. | 3 |
| C. | 27 |
| D. | 36 |
| Answer» D. 36 | |
| 754. |
The following equilibrium is established when hydrogen chloride is dissolved in acetic acid. \[HCl+C{{H}_{3}}COOH\rightleftharpoons C{{l}^{-}}+C{{H}_{3}}COOH_{2}^{+}\] The set that characterises the conjugate acid- base pairs is |
| A. | \[(HCl,C{{H}_{3}}COOH)and(C{{H}_{3}}COOH_{2}^{+},C{{l}^{-}})\] |
| B. | \[(HCl,C{{H}_{3}}COOH_{2}^{+})and(C{{H}_{3}}COOH,C{{l}^{-}})\] |
| C. | \[(C{{H}_{3}}COOH_{2}^{+},HCl)and(C{{l}^{-}},C{{H}_{3}}COOH)\] |
| D. | \[(HCl,C{{l}^{-}})and(C{{H}_{3}}COOH_{2}^{+},C{{H}_{3}}COOH)\] |
| Answer» E. | |
| 755. |
A solution of \[0.1\text{ }M\text{ }NaZ\] has \[pH=8.90.\]The \[{{K}_{a}}\] of HZ is |
| A. | \[6.3\times {{10}^{-11}}\] |
| B. | \[6.3\times {{10}^{-10}}\] |
| C. | \[1.6\times {{10}^{-5}}\] |
| D. | \[1.6\times {{10}^{-6}}\] |
| Answer» D. \[1.6\times {{10}^{-6}}\] | |
| 756. |
The solubility of \[Pb{{I}_{2}}\] at \[25{}^\circ C\] is\[0.7\text{ }g\text{ }{{L}^{-1}}\]. The solubility product of \[Pb{{I}_{2}}\] at this temperature is (molar mass of\[Pb{{I}_{2}}=461.2gmo{{l}^{-1}}\]) |
| A. | \[1.40\times {{10}^{-9}}\] |
| B. | \[0.14\times {{10}^{-9}}\] |
| C. | \[140\times {{10}^{-9}}\] |
| D. | \[14.0\times {{10}^{-9}}\] |
| Answer» E. | |
| 757. |
Consider the expression \[\Delta G=-\,RT\,\ln {{K}_{p}}+RT\,\ln {{Q}_{p}}\] and indicate the correct statement at equilibrium |
| A. | \[\Delta G=0,\text{ }{{Q}_{p}}>{{K}_{p}}\] the equilibrium reaction will shift from left to right |
| B. | \[\Delta G=0,\text{ }{{Q}_{p}}={{K}_{p}}\] the equilibrium reaction will shift from left to right |
| C. | \[\Delta G=\infty ,\text{ }{{Q}_{p}}<{{K}_{p}}\] the equilibrium reaction will shift from right to left |
| D. | \[\Delta G<0,\text{ }{{Q}_{p}}>{{K}_{p}}\] the equilibrium reaction will shift from right to left where \[{{Q}_{p}}\] and \[{{K}_{p}}\] term refer to reaction quotient and equilibrium constant at constant pressure respectively. |
| Answer» C. \[\Delta G=\infty ,\text{ }{{Q}_{p}}<{{K}_{p}}\] the equilibrium reaction will shift from right to left | |
| 758. |
\[{{K}_{1}},{{K}_{2}}\] and \[{{K}_{3}}\] are the equilibrium constants of the following reactions (I), (II) and (III) respectively:(I) \[{{N}_{2}}+2{{O}_{2}}\rightleftharpoons 2N{{O}_{2}}\](II) \[2N{{O}_{2}}\rightleftharpoons {{N}_{2}}+2{{O}_{2}}\](III) \[N{{O}_{2}}\rightleftharpoons \frac{1}{2}{{N}_{2}}+{{O}_{2}}\]The correct relation from the following is |
| A. | \[{{K}_{1}}=\frac{1}{{{K}_{2}}}=\frac{1}{{{K}_{3}}}\] |
| B. | \[{{K}_{1}}=\frac{1}{{{K}_{2}}}=\frac{1}{{{({{K}_{3}})}^{2}}}\] |
| C. | \[{{K}_{1}}=\sqrt{{{K}_{2}}}={{K}_{3}}\] |
| D. | \[{{K}_{1}}=\frac{1}{{{K}_{2}}}={{K}_{3}}\] |
| Answer» C. \[{{K}_{1}}=\sqrt{{{K}_{2}}}={{K}_{3}}\] | |
| 759. |
Which of the following is true at chemical equilibrium? |
| A. | \[{{(\Delta G)}_{T,P}}\] is minimum and \[{{(\Delta S)}_{U,V}}\] is also minimum |
| B. | \[{{(\Delta G)}_{T,V}}\]is minimum and \[{{(\Delta S)}_{U,V}}\] is maximum |
| C. | \[{{(\Delta G)}_{T,V}}\] is maximum and \[{{(\Delta S)}_{U,V}}\]is zero |
| D. | \[{{(\Delta G)}_{T,P}}\] is zero and \[{{(\Delta S)}_{U,V}}\] is also zero |
| Answer» E. | |
| 760. |
For a reversible gaseous reaction \[{{N}_{2}}+3{{H}_{2}}\rightleftharpoons 2N{{H}_{3}}\] at equilibrium, if some moles of \[{{H}_{2}}\] are replaced by same number of moles of \[{{T}_{2}}\](T is tritium, isotope of H and assume isotopes do not have different chemical properties) without affecting other parameter, then: |
| A. | the sample of ammonia obtained after sometime will be radioactive. |
| B. | moles of \[{{N}_{2}}\] after the change will be different as compared to moles of \[{{N}_{2}}\] present before the change |
| C. | the value of \[{{K}_{p}}\] or \[{{K}_{c}}\]will change |
| D. | the average molecular mass of new equilibrium will be same as that of old equilibrium |
| Answer» B. moles of \[{{N}_{2}}\] after the change will be different as compared to moles of \[{{N}_{2}}\] present before the change | |
| 761. |
For the reaction \[N{{H}_{4}}HS(g)\rightleftharpoons N{{H}_{3}}(g)+{{H}_{2}}S(g)\] in a closed flask, the equilibrium pressure is P atm. The standard free energy of the reaction would be: |
| A. | \[-RT\] ln p |
| B. | \[-RT\] (ln p - ln 2) |
| C. | \[-2RT\] ln p |
| D. | \[-2RT\] (ln p - ln 2) |
| Answer» E. | |
| 762. |
For the reaction: \[2Ba{{O}_{2}}(s)\rightleftharpoons 2BaO(s)+{{O}_{2}}(g);\] \[\Delta H=+ve.\] In equilibrium condition, pressure of \[{{O}_{2}}\] is dependent on |
| A. | mass of \[Ba{{O}_{2}}\] |
| B. | mass of \[BaO\] |
| C. | temperature of equilibrium |
| D. | mass of \[Ba{{O}_{2}}\] and \[BaO\]both |
| Answer» D. mass of \[Ba{{O}_{2}}\] and \[BaO\]both | |
| 763. |
The reaction, \[S{{O}_{2}}+C{{l}_{2}}\xrightarrow{{}}S{{O}_{2}}C{{l}_{2}}\] is exothermic and reversible. A mixture of\[SO{{ }_{2}}(g)\], \[C{{l}_{2}}(g)\] and \[S{{O}_{2}}C{{l}_{2}}(l)\] is at equilibrium in a closed container. Now a certain quantity of extra \[S{{O}_{2}}\]is introduced into the container, the volume remaining the same. Which of the following is/ are true? |
| A. | The pressure inside the container will not change. |
| B. | The temperature will not change. |
| C. | The temperature will increase. |
| D. | The temperature will decrease. |
| Answer» D. The temperature will decrease. | |
| 764. |
On the basis of Le-Chatelier's principle, predict which of the following conditions would be unfavourable for the formation of 803? Given that \[2S{{O}_{2}}+O\rightleftharpoons 2S{{O}_{3}};\Delta H=-42kcal\] |
| A. | Low pressure and low temperature |
| B. | High pressure and low temperature |
| C. | High temperature and low pressure |
| D. | High concentration of \[S{{O}_{2}}\] |
| Answer» D. High concentration of \[S{{O}_{2}}\] | |
| 765. |
(1) \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g),{{K}_{1}}\](2) \[{{N}_{2}}(g)+{{O}_{2}}(g)\rightleftharpoons 2NO(g),{{K}_{2}}\](3) \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\rightleftharpoons {{H}_{2}}O(g),{{K}_{3}}\]The equation for the equilibrium constant of the reaction\[2N{{H}_{3}}(g)+\frac{5}{2}{{O}_{2}}(g)\rightleftharpoons 2NO(g)+3{{H}_{2}}O(g),\]\[({{K}_{4}})\] in terms of \[{{K}_{1}},{{K}_{2}}\] and\[~{{K}_{3}}\] is: |
| A. | \[\frac{{{K}_{1}}.{{K}_{2}}}{{{K}_{3}}}\] |
| B. | \[\frac{{{K}_{1}}.K_{3}^{2}}{{{K}_{2}}}\] |
| C. | \[{{K}_{1}}{{K}_{2}}{{K}_{3}}\] |
| D. | \[\frac{{{K}_{2}}.K_{3}^{3}}{{{K}_{1}}}\] |
| Answer» E. | |
| 766. |
When heated, ammonium carbamate decomposes as follows: \[N{{H}_{4}}COON{{H}_{2}}(s)\rightleftharpoons 2N{{H}_{3}}(g)+C{{O}_{2}}(g)\]. At a certain temperature, the equilibrium pressure of the system is 0.318 atm. \[{{K}_{p}}\] for the reaction is: |
| A. | 0.128 |
| B. | 0.426 |
| C. | \[4.76\times {{10}^{-3}}\] |
| D. | None of these |
| Answer» D. None of these | |
| 767. |
The standard state Gibb's free energy change for the isomerisation reaction \[cis-2-pentene\rightleftharpoons trans-2-pentene\]is \[-3.67\text{ }kJ\text{ }mo{{l}^{-1}}\] at 400 K. If more trans-2-pentene is added to the reaction vessel |
| A. | more cis-2-pentene is formed |
| B. | equilibrium shifts in the forward direction |
| C. | equilibrium remains unaltered |
| D. | more trans-2-pentene is produced |
| Answer» B. equilibrium shifts in the forward direction | |
| 768. |
Some inert gas is added at constant volume to the following reaction at equilibrium \[N{{H}_{4}}HS(s)\rightleftharpoons N{{H}_{3}}(g)+{{H}_{2}}S(g)\] Predict the effect of adding the inert gas: |
| A. | The equilibrium shifts in the forward direction |
| B. | The equilibrium shifts in the backward direction |
| C. | The equilibrium remains unaffected |
| D. | The value of \[{{K}_{p}}\]is increased |
| Answer» D. The value of \[{{K}_{p}}\]is increased | |
| 769. |
At a certain temperature, only 50% HI is dissociated into \[{{H}_{2}}\] and \[{{I}_{2}}\] at equilibrium. The equilibrium constant is: |
| A. | 1.0 |
| B. | 3.0 |
| C. | 0.5 |
| D. | 0.25 |
| Answer» B. 3.0 | |
| 770. |
At \[527{}^\circ C\], the reaction given below has \[{{K}_{c}}=4\] \[N{{H}_{3}}(g)\rightleftharpoons \frac{1}{2}{{N}_{2}}(g)+\frac{3}{2}{{H}_{2}}(g)\] What is the \[{{K}_{p}}\] for the reaction? \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g)\] |
| A. | \[16\times {{(800R)}^{2}}\] |
| B. | \[{{\left( \frac{800R}{4} \right)}^{-2}}\] |
| C. | \[{{\left( \frac{1}{4\times 800R} \right)}^{2}}\] |
| D. | None of these |
| Answer» D. None of these | |
| 771. |
\[28g\,{{N}_{2}}\] and 6.0 g of \[{{H}_{2}}\] are heated over catalyst in a closed one litre flask of\[450{}^\circ C\]. The entire equilibrium mixture required 500 mL of 1.0 M \[{{H}_{2}}S{{O}_{4}}\] for neutralisation. The value of \[{{K}_{c}}\] for the reaction \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g)\] is |
| A. | \[0.06\text{ }mo{{l}^{-2}}{{L}^{2}}\] |
| B. | \[0.59\text{ }mo{{l}^{-2}}{{L}^{2}}\] |
| C. | \[1.69\text{ }mo{{l}^{2}}{{L}^{-2}}\] |
| D. | \[0.03\text{ }mo{{l}^{2}}{{L}^{-2}}\] |
| Answer» C. \[1.69\text{ }mo{{l}^{2}}{{L}^{-2}}\] | |
| 772. |
If \[CuS{{O}_{4}}.5{{H}_{2}}O(s)\rightleftharpoons \] \[CuS{{O}_{4}}.3{{H}_{2}}O\left( s \right)+2{{H}_{2}}O\left( g \right)\] \[{{K}_{p}}=1.086\times {{10}^{-4}}at{{m}^{2}}\] at \[25{}^\circ C\]. The efflorescent nature of \[CuS{{O}_{4}}.5{{H}_{2}}O\] can be noticed when the vapour pressure of \[{{H}_{2}}O\] in atmosphere is |
| A. | >9.72mm |
| B. | <7.92mm |
| C. | >7.92mm |
| D. | < 11.92mm |
| Answer» C. >7.92mm | |
| 773. |
The value of \[{{K}_{p}}\] for the equilibrium reaction \[{{N}_{2}}{{O}_{4}}(g)\rightleftharpoons 2N{{O}_{2}}(g)\] is 2. The percentage dissociation of \[{{N}_{2}}{{O}_{4}}(g)\] at a pressure of 0.5 atm is |
| A. | 25 |
| B. | 88 |
| C. | 50 |
| D. | 71 |
| Answer» E. | |
| 774. |
Gaseous \[{{N}_{2}}{{O}_{4}}\] dissociates into gaseous \[N{{O}_{2}}\]according to the reaction \[[{{N}_{2}}{{O}_{4}}(g)\rightleftharpoons 2N{{O}_{2}}(g)]\] At 300 K and 1 atm pressure, the degree of dissociation of \[{{N}_{2}}{{O}_{4}}\] is 0.2. If one mole of \[{{N}_{2}}{{O}_{4}}\] gas is contained in a vessel, then the density of the equilibrium mixture is: |
| A. | 1.56 g/L |
| B. | 6.22 g/L |
| C. | 3.11g/L |
| D. | 4.56 g/L |
| Answer» D. 4.56 g/L | |
| 775. |
\[{{K}_{c}}\] for \[PC{{l}_{5}}(g)\rightleftharpoons PC{{l}_{3}}(g)+C{{l}_{2}}(g)\] is 0.04 at \[250{}^\circ C\]. How many moles of \[PC{{l}_{5}}\] must be added to a 3 L flask to obtain a \[C{{l}_{2}}\] concentration of 0.15M |
| A. | 4.2 moles |
| B. | 2.1 moles |
| C. | 5.5 moles |
| D. | 6.3 moles |
| Answer» C. 5.5 moles | |
| 776. |
The equilibrium constant for the reaction \[W+X\rightleftharpoons Y+Z\] is 9.Ifone mole of each of w and x are mixed and there is no change in volume, the number of moles of y formed is |
| A. | 0.10 |
| B. | 0.50 |
| C. | 0.75 |
| D. | 0.54 |
| Answer» D. 0.54 | |
| 777. |
Sum of first three ionization energies of Al is \[53.0\text{ }eV\text{ }ato{{m}^{-1}}\] and the sum of first two ionization energies of Na is \[52.2\text{ }eV\text{ }ato{{m}^{-1}}.\] Out of Al(III) and Na(II) |
| A. | Na (II) is more stable than Al (III) |
| B. | Al (III) is more stable than Na (II) |
| C. | Both are equally stable |
| D. | Both are equally unstable |
| Answer» C. Both are equally stable | |
| 778. |
In the long form of the periodic table, the valence shell electronic configuration of \[5{{s}^{2}}5{{p}^{4}}\] corresponds to the element present in: |
| A. | Group 16 and period 6 |
| B. | Group 17 and period 6 |
| C. | Group 16 and period 5 |
| D. | Group 17 and period 5 |
| Answer» D. Group 17 and period 5 | |
| 779. |
Consider the following ionisation reactions:I.E.\[\left( kJ\text{ }mo{{l}^{-1}} \right)\] I.E. \[\left( kJ\text{ }mo{{l}^{-1}} \right)\]\[A(g)\to {{A}^{+}}(g)+{{e}^{-}},\,\,{{A}_{1}}\,\,A(g)~\to {{A}^{+}}(g)+{{e}^{-}},\,\,{{A}_{1}}\]\[{{B}^{+}}(g)\to {{B}^{2+}}(g)+{{e}^{-}},\,\,{{B}_{2}}C(g)\to {{C}^{+}}(g)+{{e}^{-}},\,\,{{C}_{1}}\]\[{{C}^{+}}(g)\to {{C}^{2+}}(g)+{{e}^{-}},\,\,{{C}_{1}}\,{{C}^{2+}}(g)\to {{C}^{3+}}(g)+{{e}^{-}},\,\,{{C}_{3}}\]If monovalent positive ion of A, divalent positive ion of B and trivalent positive ion of C have zero electron. Then incorrect order of corresponding I.E. is: |
| A. | \[{{C}_{3}}>{{B}_{2}}>{{A}_{1}}\] |
| B. | \[{{B}_{1}}>{{A}_{1}}>{{C}_{1}}\] |
| C. | \[{{C}_{3}}>{{C}_{2}}>{{B}_{2}}\] |
| D. | \[{{B}_{2}}>{{C}_{3}}>{{A}_{1}}\] |
| Answer» E. | |
| 780. |
Similarity in chemical properties of the atoms of elements in a group of the Periodic table is most closely related to: |
| A. | atomic numbers |
| B. | atomic masses |
| C. | number of principal energy levels |
| D. | number of valence electrons |
| Answer» B. atomic masses | |
| 781. |
Which ionisation potential (IP) in the following equations involves the greatest amount of energy? |
| A. | \[Na\to N{{a}^{+}}+{{e}^{-}}\] |
| B. | \[{{K}^{+}}\to {{K}^{2+}}+{{e}^{-}}\] |
| C. | \[{{C}^{2+}}\to {{C}^{3+}}+{{e}^{-}}\] |
| D. | \[C{{a}^{+}}\to C{{a}^{2+}}+{{e}^{-}}\] |
| Answer» C. \[{{C}^{2+}}\to {{C}^{3+}}+{{e}^{-}}\] | |
| 782. |
If the ionization enthalpy and electron gain enthalpy of an element are 275 and\[86\text{ }kcal\text{ }mo{{l}^{-1}}\] respectively, then the electronegativity of the element on the Pauling scale is: |
| A. | 2.8 |
| B. | 0.0 |
| C. | 4.0 |
| D. | 2.6 |
| Answer» B. 0.0 | |
| 783. |
The basic character of \[MgO,\text{ }BaO,\text{ }N{{a}_{2}}O\] and \[FeO\]follow the order |
| A. | \[MgO<FeO<BaO<N{{a}_{2}}O\] |
| B. | \[FeO<MgO<N{{a}_{2}}O<BaO\] |
| C. | \[FeO<MgO<BaO<N{{a}_{2}}O\] |
| D. | \[N{{a}_{2}}O<MgO<FeO<BaO\] |
| Answer» D. \[N{{a}_{2}}O<MgO<FeO<BaO\] | |
| 784. |
Which one of the following ionic species has the greatest proton affinity to form stable compound? |
| A. | \[C{{l}^{-}}\] |
| B. | \[{{F}^{-}}~\] |
| C. | \[~{{I}^{-}}\] |
| D. | \[~B{{r}^{-}}\] |
| Answer» C. \[~{{I}^{-}}\] | |
| 785. |
Electron affinity is positive for |
| A. | \[O(g)+{{e}^{-}}\to {{O}^{-}}(g)\] |
| B. | \[S(g)+{{e}^{-}}\to {{S}^{-}}(g)\] |
| C. | \[{{O}^{+}}(g)+{{e}^{~}}^{-}\to O(g)\] |
| D. | \[{{O}^{-}}(g)+{{e}^{-}}\to {{O}^{2-}}(g)\] |
| Answer» E. | |
| 786. |
Consider the following information about element P and Q: Period numberGroup numberP215Q32 |
| A. | QP |
| B. | \[{{Q}_{2}}{{P}_{3}}\] |
| C. | \[{{Q}_{3}}{{P}_{2}}\] |
| D. | \[{{Q}_{2}}P\] |
| Answer» D. \[{{Q}_{2}}P\] | |
| 787. |
Which of the following order is wrong? |
| A. | \[N{{H}_{3}}<P{{H}_{3}}<As{{H}_{3}}-Acidic\] |
| B. | \[Li<Be<B<C-I{{E}_{1}}\] |
| C. | \[A{{l}_{2}}{{O}_{3}}<MgO<N{{a}_{2}}O<{{K}_{2}}O-Basic\] |
| D. | \[L{{i}^{+}}<N{{a}^{+}}<{{K}^{+}}<C{{s}^{+}}-\]Ionic radius |
| Answer» C. \[A{{l}_{2}}{{O}_{3}}<MgO<N{{a}_{2}}O<{{K}_{2}}O-Basic\] | |
| 788. |
The electronic configuration of an element is. The atomic number and the group number of the element 'X' which is just below the above element in the periodic table are respectively |
| A. | 23 and 5 |
| B. | 23 and 15 |
| C. | 33 and 15 |
| D. | 33 and 5 |
| Answer» D. 33 and 5 | |
| 789. |
Highest electron affinity is shown by |
| A. | \[{{O}^{-}}\] |
| B. | \[{{F}^{-}}\] |
| C. | \[C{{l}_{2}}\] |
| D. | \[~{{F}_{2}}\] |
| Answer» B. \[{{F}^{-}}\] | |
| 790. |
Which one of the following statements is incorrect in relation to ionisation enthalpy? |
| A. | Ionisation enthalpy increases for each successive electron. |
| B. | The greatest increase in ionisation enthalpy is experienced on removal of electron from core noble gas configuration. |
| C. | End of valence electrons is marked by a big jump in ionisation enthalpy. |
| D. | Removal of electron from orbitals bearing lower n value is easier than from orbital having higher n value. |
| Answer» E. | |
| 791. |
The first ionisation potential of aluminium is smaller than that of magnesium because |
| A. | Atomic size of Al > Atomic size of Mg. |
| B. | Atomic size of Al < Atomic size of Mg. |
| C. | Al has one electron in p - orbital |
| D. | None of these |
| Answer» D. None of these | |
| 792. |
The electronegativity follows the order |
| A. | \[F>O>Cl>Br\] |
| B. | \[~F>Cl>Br>O\] |
| C. | \[~O>F>Cl>Br\] |
| D. | \[~Cl>F>O>Br\] |
| Answer» B. \[~F>Cl>Br>O\] | |
| 793. |
Which of the following ionisation energy values for calcium show a sudden increase? |
| A. | Third |
| B. | Second |
| C. | First |
| D. | Fourth |
| Answer» B. Second | |
| 794. |
Which of the following is not the correct order for the stated property? |
| A. | \[Ba>Sr>\]Mg; atomic radius |
| B. | \[F>O>N:\] first ionization enthalpy |
| C. | \[Cl>F>I;\] electron affinity |
| D. | \[O>Se>Te;\] electronegativity |
| Answer» C. \[Cl>F>I;\] electron affinity | |
| 795. |
Which among the following elements has the highest first ionization enthalpy? |
| A. | Nitrogen |
| B. | Boron |
| C. | Carbon |
| D. | Oxygen |
| Answer» B. Boron | |
| 796. |
In which of the following arrangements, the sequence is not strictly according to the property written against it? |
| A. | \[C{{O}_{2}}<Si{{O}_{2}}<Sn{{O}_{2}}<Pb{{O}_{2}}\]: increasing oxidising power |
| B. | \[N{{H}_{3}}<P{{H}_{3}}<As{{H}_{3}}<Sb{{H}_{3}}:\] increasing basic strength |
| C. | \[HF<HCl<HBr<HI:\] increasing acid strength |
| D. | \[B<C<O<N:\] increasing first ionisation enthalpy. |
| Answer» C. \[HF<HCl<HBr<HI:\] increasing acid strength | |
| 797. |
Ionization energies of atoms A and B are 400 and \[300\text{ }k\text{ }cal\text{ }mo{{l}^{-1}}\] respectively. The electron affinities of these atoms are 80.0 and \[85.0\text{ }k\text{ }cal\,mo{{l}^{-1}}\] respectively. Then which is the correct statement regarding electronegativity\[\chi \]? |
| A. | \[{{\chi }_{A}}<{{\chi }_{B}}\] |
| B. | \[{{\chi }_{A}}>{{\chi }_{B}}\] |
| C. | \[{{\chi }_{A}}={{\chi }_{B}}\] |
| D. | none of these |
| Answer» C. \[{{\chi }_{A}}={{\chi }_{B}}\] | |
| 798. |
The electron affinity of chlorine is 3.7 eV. 1 g of chlorine is completely converted to \[C{{l}^{-}}\]ion in a gaseous state.\[\left( 1\text{ }eV=23.06\,Kcal\text{ }mo{{l}^{-1}} \right)\]. Energy released in the process is |
| A. | 4.8 kcal |
| B. | 7.2 kcal |
| C. | 8.2 kcal |
| D. | 2.4 kcal |
| Answer» E. | |
| 799. |
Consider the following four elements, which are represented according to long form of periodic table. Here W, Y and Z are left, up and right elements with respect to the element 'X' and 'X' belongs to 16th group and 3rd period. Then according to given information the incorrect statement regarding given elements is: |
| A. | Maximum electronegativity: Y |
| B. | Maximum catenation property: X |
| C. | Maximum electron affinity: Z |
| D. | Y exhibits variable covalency |
| Answer» E. | |
| 800. |
The van der Waal and covalent radii of fluorine atom respectively from the following figure are. |
| A. | 219 pm, 72 pm |
| B. | 75 pm, 72 pm |
| C. | 147 pm, 72 pm |
| D. | 147 pm, 144 pm |
| Answer» D. 147 pm, 144 pm | |