Some Basic Concepts of Chemistry Set-2

Practice Important MCQs for Some Basic Concepts of Chemistry — Chemistry, Class 11.

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Q1. If the moles of the solute are cancelled out by the total number of moles, the resulting quantity is:

(A)

Molality

(B)

Molarity

(C)

Mole fraction

(D)

Percentage by volume

Q2. What is the standard $\text{SI}$ unit of time?

(A)

Minute

(B)

Hour

(C)

Second

(D)

Day

Q3. Which law states that equal volumes of gases at the same temperature and pressure should contain equal number of molecules?

(A)

Law of definite proportions

(B)

Law of multiple proportions

(C)

Law of conservation of mass

(D)

Avogadro law

Q4. How many moles of water are present in $180\text{ grams of water } (\text{H}_2\text{O})$ ?

(A)

$5\text{ mol}$

(B)

$1\text{ mol}$

(C)

$10\text{ mol}$

(D)

$18\text{ mol}$

Q5. How many molecules are present in $10\text{ moles of water}$ ?

(A)

$6.023 \times 10^{23}$ molecules

(B)

$6.023 \times 10^{24}$ molecules

(C)

$10$ molecules

(D)

$10 \times 6.022 \times 10^{23}$ atoms

Q6. If a solution contains $10\text{g of } \text{NaOH}$ (Molar Mass $= 40\text{ g/mol}$ ) dissolved in $100\text{g of water}$ , what is the number of moles of $\text{NaOH}$ ?

(A)

$0.25\text{ mol}$

(B)

$0.1\text{ mol}$

(C)

$0.5\text{ mol}$

(D)

$1\text{ mol}$

Q7. If the molality of an aqueous solution is $1\text{m}$ , what is the mass of the solvent (water)?

(A)

$1\text{ L}$

(B)

$100\text{ g}$

(C)

$1000\text{ g}$

(D)

$10\text{ g}$

Q8. The volume of pure water required to have a mass of $1000\text{ grams}$ is: (Density $1\text{ g/mL}$ )

(A)

$100\text{ mL}$

(B)

$1000\text{ mL}$

(C)

$1\text{ L}$

(D)

Both (2) and (3)

Q9. The relationship used when mixing two solutions (A and B) of the same substance to find the final molarity ( $M_F$ ) and final volume ( $V_F$ ) is:

(A)

$M_1V_1 + M_2V_2 = M_F / V_F$

(B)

$M_1V_1 / M_2V_2 = M_F / V_F$

(C)

$M_1V_1 + M_2V_2 = M_F V_F$

(D)

$M_1V_1 - M_2V_2 = M_F V_F$

Q10. What is the molar mass of Copper Sulphate $(\text{CuSO}_4)$ ? (Atomic weight $\text{Cu} = 63.5, \text{ S} = 32, \text{ O} = 16$ )

(A)

$159.5\text{ g/mol}$

(B)

$120\text{ g/mol}$

(C)

$95.5\text{ g/mol}$

(D)

$180\text{ g/mol}$

Q11. What is the value of $1$ divided by Avogadro's number ( $6.022 \times 10^{23}$ )?

(A)

$1.66 \times 10^{24}$

(B)

$1.99 \times 10^{-23}$

(C)

$1.66 \times 10^{-24}$

(D)

$1.66 \times 10^{-23}$

Q12. In the context of Dalton's theory, the concept that different elements combine in a fixed ratio primarily supports:

(A)

Law of Conservation of Mass

(B)

Law of Definite Proportions

(C)

Avogadro's Law

(D)

Law of Multiple Proportions

Q13. Which quantity relates Molecular Weight ( $\text{M.W.}$ ) to Vapour Density ( $\text{V.D.}$ )?

(A)

$\text{M.W.} = \text{V.D.}$

(B)

$\text{M.W.} = \text{V.D.} + 2$

(C)

$\text{M.W.} = 2 \times \text{V.D.}$

(D)

$\text{M.W.} = \text{V.D.} / 2$

Q14. If the density of a solution is $3.12\text{ g mL}^{-1}$ and the volume is $1.5\text{ mL}$ , the mass of the solution calculated in significant figures is:

(A)

$4.7\text{ g}$

(B)

$4680 \times 10^{-3}\text{ g}$

(C)

$4.680\text{ g}$

(D)

$46.80\text{ g}$

Q15. The ratio of masses of oxygen which combines with $1\text{g of element X}$ , if $\text{X}$ forms two oxides, $\text{XO}$ ( $50\%\text{ O}$ ) and $\text{XO}_2$ ( $60\%\text{ O}$ ), is $2:3$ . This observation supports which law?

(A)

Law of definite proportions

(B)

Law of conservation of mass

(C)

Law of multiple proportions

(D)

Avogadro law

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