Most Important Questions For Class 12th CBSE

Most Important Questions of All The Chaptar of Class 12th Below are the important questions along with the answers .These questions are most asked in the recent school exams. These are totally based on the CBSE board curriculum. We recommend everyone, do not skip these questions.

Important Questions of All The Chaptar of Class 12th

Solution

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1 Which of the following solutions will have the highest conductivity at 298 K 298 K 298K298 \mathrm{~K}298 K ?
(a) 0.01 M H C l 0.01 M H C l 0.01MHCl0.01 \mathrm{MHCl}0.01MHCl solution
(b) 0.1 M H C l 0.1 M H C l 0.1MHCl0.1 \mathrm{MHCl}0.1MHCl solution
(c) 0.01 M C H 3 C O O H 0.01 M C H 3 C O O H 0.01MCH_(3)COOH0.01 \mathrm{MCH}_3 \mathrm{COOH}0.01MCH3COOH solution
(d) 0.1 M C H 3 C O O H 0.1 M C H 3 C O O H 0.1MCH_(3)COOH0.1 \mathrm{MCH}_3 \mathrm{COOH}0.1MCH3COOH solution
2 A 5 % 5 % 5%5 \%5% solution of N a 2 S O 4 1 H 2 O ( M W = 322 ) N a 2 S O 4 1 H 2 O ( M W = 322 ) Na_(2)SO_(4)*1H_(2)O(MW=322)\mathrm{Na}_2 \mathrm{SO}_4 \cdot 1 \mathrm{H}_2 \mathrm{O}(\mathrm{MW}=322)Na2SO41H2O(MW=322) is isotonic with 2 % 2 % 2%2 \%2% solution of non- electrolytic, non volatile substance X X XXX. Find out the molecular weight of X X XXX.
3 Answer the following questions:
a. State Henry's law and explain why are the tanks used by scuba divers filled with air diluted with helium ( 11.7 % 11.7 % 11.7%11.7 \%11.7% helium, 56.2 % 56.2 % 56.2%56.2 \%56.2% nitrogen and 32.1 % 32.1 % 32.1%32.1 \%32.1% oxygen)?
b. Assume that argon exerts a partial pressure of 6 bar. Calculate the solubility of argon gas in water.
(Given Henry's law constant for argon dissolved in water, K H = 40 k b a r K H = 40 k b a r K_(H)=40kbar\mathrm{K}_{\mathrm{H}}=40 \mathrm{kbar}KH=40kbar )

Electrochemistry

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  1. Given below are two statements labelled as Assertion (A) and Reason (R)
    Assertion (A): During electrolysis of aqueous copper sulphate solution using copper electrodes hydrogen gas is released at the cathode.
    Reason (R): The electrode potential of C u 2 + / C u C u 2 + / C u Cu^(2+)//Cu\mathrm{Cu}^{2+} / \mathrm{Cu}Cu2+/Cu is greater than that of H + / H 2 H + / H 2 H+//H_(2)\mathrm{H}+/ \mathrm{H}_2H+/H2
    Select the most appropriate answer from the options given below:
    (a) Both A A AAA and R R RRR are true and R R RRR is the correct explanation of A A AAA
    (b) Both A A AAA and R R RRR are true but R R RRR is not the correct explanation of A A AAA.
    (c) A A AAA is true but R R RRR is false.
    (d) A A AAA is false but R R RRR is true.
  2. (a) Can we construct an electrochemical cell with two half-cells composed of Z n S O 4 Z n S O 4 ZnSO_(4)\mathrm{ZnSO}_4ZnSO4 solution and zinc electrodes? Explain your answer.
    (b) Calculate the λ 0 m λ 0 m lambda^(0)m\lambda^0 \mathrm{~m}λ0 m for C l C l Cl\mathrm{Cl}Cl - ion from the data given below:
Λ 0 m M g C l 2 = 258.6 S c m 2 m o l 1 and λ 0 m M g 2 + = 106 S c m 2 m o l 1 Λ 0 m M g C l 2 = 258.6 S c m 2 m o l 1  and  λ 0 m M g 2 + = 106 S c m 2 m o l 1 Lambda^(0)mMgCl2=258.6Scm^(2)mol^(-1)" and "lambda^(0)mMg^(2+)=106Scm^(2)mol^(-1)\Lambda^0 \mathrm{mMgCl} 2=258.6 \mathrm{Scm}^2 \mathrm{~mol}^{-1} \text { and } \lambda^0 \mathrm{mMg}^{2+}=106 \mathrm{Scm}^2 \mathrm{~mol}^{-1}Λ0mMgCl2=258.6Scm2 mol1 and λ0mMg2+=106Scm2 mol1
(c) The cell constant of a conductivity cell is 0.146 c m 1 0.146 c m 1 0.146cm^(-1)0.146 \mathrm{~cm}^{-1}0.146 cm1. What is the conductivity of 0.01 M 0.01 M 0.01M0.01 \mathrm{M}0.01M solution of an electrolyte at 298 K 298 K 298K298 \mathrm{~K}298 K, if the resistance of the cell is 1000 o h m 1000 o h m 1000ohm1000 \mathrm{ohm}1000ohm ?
3. The molar conductivity of C H 3 C O O H C H 3 C O O H CH_(3)COOH\mathrm{CH}_3 \mathrm{COOH}CH3COOH at infinite dilution is 390 S c m 2 / m o l 390 S c m 2 / m o l 390Scm^(2)//mol390 \mathrm{Scm}^2 / \mathrm{mol}390Scm2/mol. Using the graph and given information, the molar conductivity of C H 3 C O O K C H 3 C O O K CH_(3)COOK\mathrm{CH}_3 \mathrm{COOK}CH3COOK will be:
a. 100 S c m 2 / m o l 100 S c m 2 / m o l 100Scm^(2)//mol100 \mathrm{Scm}^2 / \mathrm{mol}100Scm2/mol
b. 115 S c m 2 / m o l 115 S c m 2 / m o l 115Scm^(2)//mol115 \mathrm{Scm}^2 / \mathrm{mol}115Scm2/mol
c. 150 S c m 2 / m o l 150 S c m 2 / m o l 150Scm^(2)//mol150 \mathrm{Scm}^2 / \mathrm{mol}150Scm2/mol
d. 125 S c m 2 / m o l 125 S c m 2 / m o l 125Scm^(2)//mol125 \mathrm{Scm}^2 / \mathrm{mol}125Scm2/mol
math

Chemical Kinetics

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1 Which of the following statement is true?
(a) molecularity of reaction can be zero or a fraction.
(b) molecularity has no meaning for complex reactions.
(c) molecularity of a reaction is an experimental quantity
(d) reactions with the molecularity three are very rare but are fast.
2 If the initial concentration of substance A A AAA is 1.5 M 1.5 M 1.5M1.5 \mathrm{M}1.5M and after 120 seconds the concentration of substance A A AAA is 0.75 M 0.75 M 0.75M0.75 \mathrm{M}0.75M, the rate constant for the reaction if it follows zero - order kinetics is:
(a) 0.00625 m o l L 1 s 1 0.00625 m o l L 1 s 1 0.00625molL^(-1)s^(-1)0.00625 \mathrm{molL}^{-1} \mathrm{~s}^{-1}0.00625molL1 s1
(b) 0.00625 s 1 0.00625 s 1 0.00625s^(-1)0.00625 \mathrm{~s}^{-1}0.00625 s1
(c) 0.00578 m o l L 1 s 1 0.00578 m o l L 1 s 1 0.00578molL^(-1)s^(-1)0.00578 \mathrm{molL}^{-1} \mathrm{~s}^{-1}0.00578molL1 s1
(d) 0.00578 s 1 0.00578 s 1 0.00578s^(-1)0.00578 \mathrm{~s}^{-1}0.00578 s1
3 a. Radioactive decay follows first - order kinetics. The initial amount of two radioactive elements X X XXX and Y Y YYY is 1 g m 1 g m 1gm1 \mathrm{gm}1gm each. What will be the ratio of X X XXX and Y Y YYY after two days if their halflives are 12 hours and 16 hours respectively?
b. The hypothetical reaction P + Q R P + Q R P+Q rarr RP+Q \rightarrow RP+QR is half order w.r.t ' P P PPP ' and zero order w.r.t ' Q Q QQQ '. What is the unit of rate constant for this reaction?

D and F block

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1 Match the properties with the elements of 3 d 3 d 3d3 d3d series:
(i) lowest enthalpy of atomization
(p) Sc
(ii) shows maximum number of oxidation states
(q) M n M n Mn\mathrm{Mn}Mn
(iii) transition metal that does not form coloured compounds
(r) Z n Z n Zn\mathrm{Zn}Zn
(s) T i T i Ti\mathrm{Ti}Ti
(a) (i) (r), (ii) (q), (iii) (p)
(b) (i) (r), (ii) (s), (iii) (p)
(c) (i) (p), (ii) (q), (iii) (r)
(d) (i) (s), (ii) (r), (iii) (p)
2 The trend of which property is represented by the following graph?
(a) ionization enthalpy
(b) atomic radii
(c) enthalpy of atomization
(d) melting point
3 Which of the following is not considered a transition element?
(a) Scandium
(b) Silver
(c) Vanadium
(d) Zinc
d and f

Coordination Compounds

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1 (a) Write the formula for the following coordination compound
Bis(ethane-1,2-diamine) dihydroxidochromium(III) chloride
(b) Does ionization isomer for the following compound exist? Justify your answer. H g [ C o ( S C N ) 4 ] H g C o ( S C N ) 4 Hg[Co(SCN)_(4)]\mathrm{Hg}\left[\mathrm{Co}(\mathrm{SCN})_4\right]Hg[Co(SCN)4]
(c) Is the central metal atom in coordination complexes a Lewis acid or a Lewis base? Explain.
2 The CFSE of [ C o C l 6 ] 3 C o C l 6 3 [CoCl_(6)]^(3-)\left[\mathrm{CoCl}_6\right]^{3-}[CoCl6]3 is 18000 c m 1 18000 c m 1 18000cm^(-1)18000 \mathrm{~cm}^{-1}18000 cm1 the CFSE for [ C o C l 4 ] C o C l 4 [CoCl_(4)]^(-)\left[\mathrm{CoCl}_4\right]^{-}[CoCl4]will be:
a. 18000 c m 1 18000 c m 1 18000cm^(-1)18000 \mathrm{~cm}^{-1}18000 cm1
b. 8000 c m 1 8000 c m 1 8000cm^(-1)8000 \mathrm{~cm}^{-1}8000 cm1
c. 2000 c m 1 2000 c m 1 2000cm^(-1)2000 \mathrm{~cm}^{-1}2000 cm1
d. 16000 c m 1 16000 c m 1 16000cm^(-1)16000 \mathrm{~cm}^{-1}16000 cm1
3 The number of ions formed on dissolving one molecule of F e S O 4 ( N H 4 ) 2 S O 4 6 H 2 C F e S O 4 N H 4 2 S O 4 6 H 2 C FeSO_(4)*(NH_(4))_(2)SO_(4)*6H_(2)C\mathrm{FeSO}_4 \cdot\left(\mathrm{NH}_4\right)_2 \mathrm{SO}_4 \cdot 6 \mathrm{H}_2 \mathrm{C}FeSO4(NH4)2SO46H2C in water is:
a. 3
b. 4
c. 5
d. 6

Haloalkanes and Haloarenes

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1 (a) Arrange the isomeric dichlorobenzene in the increasing order of their boiling point and melting points.
(b) Explain why the electrophilic substitution reactions in haloarenes occur slowly and require more drastic conditions as compared to those in benzene.
2 Which one of the following compounds is more reactive towards S N 1 S N 1 S_(N)1\mathrm{S}_{\mathrm{N}} 1SN1 reaction?
a. C H 2 = C H C H 2 B r C H 2 = C H C H 2 B r CH_(2)=CHCH_(2)Br\mathrm{CH}_2=\mathrm{CHCH}_2 \mathrm{Br}CH2=CHCH2Br
b. C 6 H 5 C H 2 B r C 6 H 5 C H 2 B r C_(6)H_(5)CH_(2)Br\mathrm{C}_6 \mathrm{H}_5 \mathrm{CH}_2 \mathrm{Br}C6H5CH2Br
c. C 6 H 5 C H ( C 6 H 5 ) B r C 6 H 5 C H C 6 H 5 B r C_(6)H_(5)CH(C_(6)H_(5))Br\mathrm{C}_6 \mathrm{H}_5 \mathrm{CH}\left(\mathrm{C}_6 \mathrm{H}_5\right) \mathrm{Br}C6H5CH(C6H5)Br
d. C 6 H 5 C H ( C H 3 ) B r C 6 H 5 C H C H 3 B r C_(6)H_(5)CH(CH_(3))Br\mathrm{C}_6 \mathrm{H}_5 \mathrm{CH}\left(\mathrm{CH}_3\right) \mathrm{Br}C6H5CH(CH3)Br
3 What would be the major product of the following reaction?
C 6 H 5 C H 2 O C 6 H 5 + H B r A + B C 6 H 5 C H 2 O C 6 H 5 + H B r A + B C_(6)H_(5)-CH_(2)-OC_(6)H5+HBrrarrA+B\mathrm{C}_6 \mathrm{H}_5-\mathrm{CH}_2-\mathrm{OC}_6 \mathrm{H} 5+\mathrm{HBr} \rightarrow \mathrm{A}+\mathrm{B}C6H5CH2OC6H5+HBrA+B
a. A = C 6 H 5 C H 2 O H , B = C 6 H 6 A = C 6 H 5 C H 2 O H , B = C 6 H 6 A=C_(6)H_(5)CH_(2)OH,B=C_(6)H_(6)\mathrm{A}=\mathrm{C}_6 \mathrm{H}_5 \mathrm{CH}_2 \mathrm{OH}, \mathrm{B}=\mathrm{C}_6 \mathrm{H}_6A=C6H5CH2OH,B=C6H6
b. A = C 6 H 5 C H 2 O H , B = C 6 H 5 B r A = C 6 H 5 C H 2 O H , B = C 6 H 5 B r A=C_(6)H_(5)CH_(2)OH,B=C6H5Br\mathrm{A}=\mathrm{C}_6 \mathrm{H}_5 \mathrm{CH}_2 \mathrm{OH}, \mathrm{B}=\mathrm{C} 6 \mathrm{H} 5 \mathrm{Br}A=C6H5CH2OH,B=C6H5Br
c. A = C 6 H 5 C H 3 , B = C 6 H 5 B r A = C 6 H 5 C H 3 , B = C 6 H 5 B r A=C_(6)H_(5)CH_(3),B=C_(6)H_(5)Br\mathrm{A}=\mathrm{C}_6 \mathrm{H}_5 \mathrm{CH}_3, \mathrm{~B}=\mathrm{C}_6 \mathrm{H}_5 \mathrm{Br}A=C6H5CH3, B=C6H5Br
d. A = C 6 H 5 C H 2 B r , B = C 6 H 5 O H A = C 6 H 5 C H 2 B r , B = C 6 H 5 O H A=C_(6)H_(5)CH_(2)Br,B=C_(6)H_(5)OHA=C_6 \mathrm{H}_5 \mathrm{CH}_2 \mathrm{Br}, \mathrm{B}=\mathrm{C}_6 \mathrm{H}_5 \mathrm{OH}A=C6H5CH2Br,B=C6H5OH

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Important Questions Ch-Classification of Elements and Periodicity in Properties Class 11th

Most Important Questions Ch-Classification of Elements and Periodicity in Properties Class 11th Below are the important questions along with the answers .These questions are most asked in the recent school exams. These are totally based on the CBSE board curriculum. We recommend everyone, do not skip these questions.

Important Questions Ch-Classification of Elements and Periodicity in Properties Class 11th

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Classification of Elements and Periodicity in Propenties
Q1. How many groups and periods were there in the original Mendeleev's Periodic Table?
Q2. State the Modern Periodic Law.
Q3. What is the main features of long form of periodic table?
Q4. How many groups and periods are there in the long form of the periodic table?
Q5. Write the electronic configuration of scandium having atomic number 21.
Q6. Out of nitrogen and oxygen, which has higher value of first ionization enthalpy?
Q7. Explain the term electron gain enthalpy.
Q8. Why is the electron gain enthalpy of nitrogen is zero?
Q9. How do electronegativity of elements behave in a period?
Q10.In K K K\mathrm{K}K and K + K + K^(+)\mathrm{K}^{+}K+, which one would have larger size?
Q11.In B r B r Br\mathrm{Br}Br and B r B r Br^(-)\mathrm{Br}^{-}Br, which one would have larger size?
Q12.In O 2 O 2 O^(2-)\mathrm{O}^{2-}O2 and F F F^(-)\mathrm{F}^{-}F, which one would have larger size?
Q13.In L i + L i + Li^(+)\mathrm{Li}^{+}Li+and N a + N a + Na^(+)\mathrm{Na}^{+}Na+, which one would have larger size?
Q14.What is meant by isoelectronic species?
Q15.Arrange the following elements in the increasing order of metallic character.
Q16.Arrange the following elements in the increasing order of non-metallic character:
Q17.Predict the position of the elements in the periodic table satisfying the electron configuration
( n n n-\mathrm{n}-n 1) d 1 n s 2 d 1 n s 2 d^(1)ns^(2)d^1 n s^2d1ns2 for n = 4 n = 4 n=4n=4n=4.
Q18.Elements A, B, C, D and E E E\mathrm{E}E have the following electronic configurations:
A: 1 s 2 2 s 2 2 p 1 1 s 2 2 s 2 2 p 1 1s^(2)2s^(2)2p^(1)1 s^2 2 s^2 2 p^11s22s22p1
B: 1 s 2 2 s 2 2 p 6 3 s 2 3 p 1 1 s 2 2 s 2 2 p 6 3 s 2 3 p 1 1s^(2)2s^(2)2p^(6)3s^(2)3p^(1)1 s^2 2 s^2 2 p^6 3 s^2 3 p^11s22s22p63s23p1
C: 1 s 2 2 s 2 2 p 6 3 s 2 3 p 3 1 s 2 2 s 2 2 p 6 3 s 2 3 p 3 1s^(2)2s^(2)2p^(6)3s^(2)3p^(3)1 s^2 2 s^2 2 p^6 3 s^2 3 p^31s22s22p63s23p3
D: 1 s 2 2 s 2 2 p 6 3 s 2 3 p 5 1 s 2 2 s 2 2 p 6 3 s 2 3 p 5 1s^(2)2s^(2)2p^(6)3s^(2)3p^(5)1 s^2 2 s^2 2 p^6 3 s^2 3 p^51s22s22p63s23p5
E: 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2)1 s^2 2 s^2 2 p^6 3 s^2 3 p^6 4 s^21s22s22p63s23p64s2
Which among these will belong to the same group in the periodic table?
Q19.What would be the IUPAC name and symbol for the element with atomic number 120 ?
Q20.Write the atomic number of the element present in the third period and seventeenth group of the periodic table.
Q21.The first ionization enthalpy ( Δ i H ) Δ i H (Delta_(i)H)\left(\Delta_{\mathrm{i}} \mathrm{H}\right)(ΔiH) values of the third period elements, N a , M g N a , M g Na,Mg\mathrm{Na}, \mathrm{Mg}Na,Mg, and S i S i Si\mathrm{Si}Si are respectively 496,737 and 786 k J m o l 1 786 k J m o l 1 786kJmol^(-1)786 \mathrm{~kJ} \mathrm{~mol}^{-1}786 kJ mol1. Predict whether the first Δ j H Δ j H Delta_(j)H\Delta_{\mathrm{j}} \mathrm{H}ΔjH value for Al will be more close to 575 or 760 k J m o l 1 760 k J m o l 1 760kJmol^(-1)760 \mathrm{~kJ} \mathrm{~mol}^{-1}760 kJ mol1 Justify your answer.
Q22.Explain why first ionization enthalpy of nitrogen is
higher than that of elements on left and right hand side in the same period (i.e., carbon and oxygen).
Q23.Among the elements L i , K , C a , S L i , K , C a , S Li,K,Ca,S\mathrm{Li}, \mathrm{K}, \mathrm{Ca}, \mathrm{S}Li,K,Ca,S and K r K r Kr\mathrm{Kr}Kr, which one has the lowest first ionization enthalpy and which one has the highest first ionization enthalpy?
Q24. Which of the following pairs of elements would you expect to have lower first ionization enthalpy?
(i) C l C l Cl\mathrm{Cl}Cl or F F F\mathrm{F}F, (ii) C l C l Cl\mathrm{Cl}Cl or S S S\mathrm{S}S, (iii) K K K\mathrm{K}K or A r A r Ar\mathrm{Ar}Ar and (iv) K r K r Kr\mathrm{Kr}Kr or X e X e Xe\mathrm{Xe}Xe.
Q25.Second and third ionization enthalpies of an element are always greater than its first ionization enthalpy. Explain.
Q26.Electron gain enthalpy values of inert gases are zero. Why?
Q27.Electron gain enthalpy of halogens are high? Explain.
Q28.Define the term electronegativity. Explain.
Q29.Electronegativity values of inert gases are zero. Explain.
Q30.Give the formula of a species that will be isoelectronic with the following atoms or ions: (i) N e N e Ne\mathrm{Ne}Ne (ii) C l C l Cl^(-)\mathrm{Cl}^{-}Cl(iii) C a 2 + C a 2 + Ca^(2+)\mathrm{Ca}^{2+}Ca2+ (iv) R b + R b + Rb^(+)\mathrm{Rb}^{+}Rb+.

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Important Questions Ch-Structure of Atom Class 11th

Chapter 2 Structure of Atom

Below are the important questions along with the answers . These questions are most asked in the recent school exams. These are totally based on the CBSE board curriculum. We recommend everyone, do not skip these questions

Structure of Atom Important
Questions Theory based

Q1. Define the term wavelength.

Q2. What is meant by electromagnetic nature of light?

Q3. Define the term frequency.

Q4. What is the speed of light in vacuum?

Q5. Give the significance of principal quantum number.

Q6. Give the significance of azimuthal quantum number.

Q7. Give the significance of magnetic quantum number.

Q8. Give the significance of spin quantum number.

Q10. The line spectrum observed when electrons fall from higher quantum levels to L level is referred to as (a)Balmer series (b) Lyman series (c) Paschen series (d) Brackett series

Q11. Define the term black body and black body radiation.

Q12. Explain Thomson model of atom.

Q13. Define the tern photoelectric effect.

Q14. Write the Bohr rule relating the energy difference to the frequency of radiation.

Q15. What is the energy of lowest energy level of hydrogen atom?

Q16. Write the mathematical expression of de Broglie equation.

Q17. State Aufbau principle.

Q18. State Heisenberg’s Uncertainty Principle.

Q19. State Pauli’s Exclusion Principle.

Q20. State Hund’s Rule of Maximum Multiplicity.

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Structure of Atom
Important Questions Numerical based

Q1. Calculate (a) wavenumber and (b) frequency of yellow radiation having wavelength

Q2. Derive de Buglie’s equation.

Q3. Calculate energy of one mole of photons of radiation whose frequency is

Structure of Atom

Q4. What is the wavelength of light emitted when
the electron in a hydrogen atom undergoes transition an energy level with n = 4 to an energy level with n = 2 ?

Q5. A 100-watt bulb emits monochromatic light of wavelength 400 nm. Calculate the number of photons emitted per second by the bulb.

Structure of Atom

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Important Questions Ch-Some Basic Concepts of Chemistry Class 11th

Important Questions Ch-Some Basic Concepts of Chemistry Class 11th

Chapter 1 Some Basic Concepts of Chemistry

Below are the important questions along with the answers . These questions are most asked in the recent school exams. These are totally based on the CBSE board curriculum. We recommend everyone, do not skip these questions

Some Basic Concepts of Chemistry Important Questions Theory based

Q.1. What is the SI unit of molarity?

Q.2. What is meant by significant figures?

Q.3. What are the various types of mixtures?

Q.4. Which of the following mixtures are homogeneous :

(i) wood (ii) tap water (iii) smoke (iv) soil and (v) cloud?

Q.5. Define the term gram atomic mass or gram atom.
Q.6. Define the term gram molecular mass or gram mole.
Q.7. Define the term molarity.

Q.8. Define the Lin of conserzation of mass.
Q.9. State Atogadro’s law.

Q.10. Explain Gay Lussac Law.
Q.11. Define the term empirical formula and molecular formula.

Q.12. What is a chemical equation? What are its essential features ?

Q.13. How many significant figures should be present in the answer of the following:

Important Questions

Q.14. What is the symbol for SI unit of mole? How is the mole defined?

Q.15. What is the difference between molality and molarity?

Q.16. Volume of a solution changes with temperature, then will the molality of the solution be affected by temperature? Give reason for your answer.

Q.17. Explain the use of limiting and excess reagents in a chemical reaction.

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Some Basic Concepts of Chemistry Important Questions Numerical based

Q.1. Calculate (i) the number of moles, (ii) the number of molecules and (iii) the volume of gas at STP in  of nitrogen.

Q.2. How many moles of methane are required to produce 22 gCO2 (g)  after combustion?

Q.3. The density of 3M solution of  is 1.25 gmL-1. Calculate molality of the solution.

Q.4. How many moles and how many grams of sodium chloride (NaCl) are present in 250 cm3 of a 0.500  solution?

Q5. In a reaction vessel 0.184g of NaOH is required to be added for completing the reaction. How many mL of 0.150MNaOH solution should be added for this requirement?

Some Basic Concepts of Chemistry

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