Quiz Tweek

Some Basic Concepts of Chemistry Set-2

Test your knowledge on Some Basic Concepts of Chemistry from Chemistry, Class 11.

50

Minutes

30

Questions

1 / -0

Marking Scheme

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Questions in this Quiz

Q1: If the moles of the solute are cancelled out by the total number of moles, the resulting quantity is:
  • Molality
  • Molarity
  • Mole fraction
  • Percentage by volume
Q2: What is the standard $\text{SI}$ unit of time?
  • Minute
  • Hour
  • Second
  • Day
Q3: Which law states that equal volumes of gases at the same temperature and pressure should contain equal number of molecules?
  • Law of definite proportions
  • Law of multiple proportions
  • Law of conservation of mass
  • Avogadro law
Q4: How many moles of water are present in $180\text{ grams of water } (\text{H}_2\text{O})$?
  • $5\text{ mol}$
  • $1\text{ mol}$
  • $10\text{ mol}$
  • $18\text{ mol}$
Q5: How many molecules are present in $10\text{ moles of water}$?
  • $6.023 \times 10^{23}$ molecules
  • $6.023 \times 10^{24}$ molecules
  • $10$ molecules
  • $10 \times 6.022 \times 10^{23}$ 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 $\text{NaOH}$?
  • $0.25\text{ mol}$
  • $0.1\text{ mol}$
  • $0.5\text{ mol}$
  • $1\text{ mol}$
Q7: If the molality of an aqueous solution is $1\text{m}$, what is the mass of the solvent (water)?
  • $1\text{ L}$
  • $100\text{ g}$
  • $1000\text{ g}$
  • $10\text{ g}$
Q8: The volume of pure water required to have a mass of $1000\text{ grams}$ is: (Density $1\text{ g/mL}$)
  • $100\text{ mL}$
  • $1000\text{ mL}$
  • $1\text{ L}$
  • 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:
  • $M_1V_1 + M_2V_2 = M_F / V_F$
  • $M_1V_1 / M_2V_2 = M_F / V_F$
  • $M_1V_1 + M_2V_2 = M_F V_F$
  • $M_1V_1 - M_2V_2 = M_F V_F$
Q10: What is the molar mass of Copper Sulphate $(\text{CuSO}_4)$? (Atomic weight $\text{Cu} = 63.5, \text{ S} = 32, \text{ O} = 16$)
  • $159.5\text{ g/mol}$
  • $120\text{ g/mol}$
  • $95.5\text{ g/mol}$
  • $180\text{ g/mol}$
Q11: What is the value of $1$ divided by Avogadro's number ($6.022 \times 10^{23}$)?
  • $1.66 \times 10^{24}$
  • $1.99 \times 10^{-23}$
  • $1.66 \times 10^{-24}$
  • $1.66 \times 10^{-23}$
Q12: In the context of Dalton's theory, the concept that different elements combine in a fixed ratio primarily supports:
  • Law of Conservation of Mass
  • Law of Definite Proportions
  • Avogadro's Law
  • Law of Multiple Proportions
Q13: Which quantity relates Molecular Weight ($\text{M.W.}$) to Vapour Density ($\text{V.D.}$)?
  • $\text{M.W.} = \text{V.D.}$
  • $\text{M.W.} = \text{V.D.} + 2$
  • $\text{M.W.} = 2 \times \text{V.D.}$
  • $\text{M.W.} = \text{V.D.} / 2$
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:
  • $4.7\text{ g}$
  • $4680 \times 10^{-3}\text{ g}$
  • $4.680\text{ g}$
  • $46.80\text{ g}$
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?
  • Law of definite proportions
  • Law of conservation of mass
  • Law of multiple proportions
  • Avogadro law
Q16: When rounding the number $1.386$ up to three significant figures, the result is:
  • $1.38$
  • $1.39$
  • $1.386$
  • $1.40$
Q17: When rounding the number $4.334$ up to three significant figures, the result is:
  • $4.34$
  • $4.33$
  • $4.330$
  • $4.32$
Q18: When rounding the number $2.808$ up to three significant figures, the result is:
  • $2.80$
  • $2.809$
  • $2.81$
  • $2.88$
Q19: What is the mass percent of Carbon in Carbon Dioxide $(\text{CO}_2)$?
  • $3.4\%$
  • $27.27\%$
  • $28.7\%$
  • $0.034\%$
Q20: The number of atoms present in one mole of an element is equal to Avogadro number. Which of the following contains the greatest number of atoms?
  • $4\text{g He}$
  • $46\text{g Na}$
  • $0.40\text{g Ca}$
  • $12\text{g He}$
Q21: How many atoms are present in $16\text{ grams of } \text{O}_2$?
  • $0.5\text{ N}_A$
  • $1\text{ N}_A$
  • $2\text{ N}_A$
  • $4\text{ N}_A$
Q22: How many atoms are present in $4\text{ grams of } \text{H}_2$?
  • $1\text{ N}_A$
  • $2\text{ N}_A$
  • $3\text{ N}_A$
  • $4\text{ N}_A$
Q23: How many atoms are present in $44\text{ grams of } \text{CO}_2$?
  • $1\text{ N}_A$
  • $2\text{ N}_A$
  • $3\text{ N}_A$
  • $4\text{ N}_A$
Q24: How many atoms are present in $28\text{ grams of } \text{N}_2$?
  • $1\text{ N}_A$
  • $2\text{ N}_A$
  • $3\text{ N}_A$
  • $4\text{ N}_A$
Q25: How many atoms are present in $12\text{ grams of Carbon } (\text{C})$?
  • $0.5\text{ N}_A$
  • $1\text{ N}_A$
  • $2\text{ N}_A$
  • $3\text{ N}_A$
Q26: How many atoms are present in $23\text{ grams of Sodium } (\text{Na})$?
  • $0.5\text{ N}_A$
  • $1\text{ N}_A$
  • $2\text{ N}_A$
  • $3\text{ N}_A$
Q27: If $1\text{ gram of } \text{M}_2\text{CO}_3$ produces $0.01186\text{ moles of } \text{CO}_2$, what is the approximate number of moles of $\text{M}_2\text{CO}_3$ present?
  • $0.00593\text{ mol}$
  • $0.01186\text{ mol}$
  • $0.02372\text{ mol}$
  • $0.04744\text{ mol}$
Q28: What is the molarity (concentration) of the solution represented by $0.2\text{ mol L}^{-1}$?
  • $0.2\text{ m}$
  • $0.2\text{ M}$
  • $2\text{ M}$
  • $20\text{ m}$
Q29: The molecular weight of an organic compound with empirical formula $\text{CH}_2\text{O}$ (Empirical formula mass $= 30$) is $90$. What is the value of 'n' ($\text{Molecular Mass / Empirical Formula Mass}$)?
  • $1$
  • $2$
  • $3$
  • $4$
Q30: A measured temperature on Fahrenheit scale is $200^\circ\text{F}$. What will this reading be on Celsius scale?
  • $40^\circ\text{C}$
  • $94^\circ\text{C}$
  • $93.3^\circ\text{C}$
  • $30^\circ\text{C}$