Classes

First Year Chemistry Basic Concepts


Change the way you learn with Maqsad's classes. Local examples, engaging animations, and instant video solutions keep you on your toes and make learning fun like never before!

Class 9Class 10First YearSecond Year
Mathcaret
Physicscaret
Chemistrycaret
Basic Concepts

672 Doubt Solutions

Experimental Techniques In Chemistry

1344 Doubt Solutions

Gases

2016 Doubt Solutions

Solids And Liquids

2688 Doubt Solutions

Atomic Structure

3360 Doubt Solutions

Chemical Bonding

4032 Doubt Solutions

ThermoChemistry

4704 Doubt Solutions

Chemical Equilibrium

5376 Doubt Solutions

Solutions

6048 Doubt Solutions

Electrochemistry

6720 Doubt Solutions

Reaction Kinetics

7392 Doubt Solutions

Q.6 Silver has atomic number 47 and has 16 known isotopes but two occur naturally i.e. Ag-107 and \mathrm{Ag}-109 . Given the following mass spectrometric data calculate the average atomic mass of silver.\begin{tabular}{|l|c|c|}\hline Isotopes & Mass (\mathrm{amu}) & Percentage abundance \\\hline { }^{107} \mathrm{Ag} & 106.90509 & 51.84 \\ { }^{100} \mathrm{Ag} & 108.90476 & 48.16 \\\hline\end{tabular}
Q.16 Ethylene glycol is used as automobile antifreeze. It has 38.7 \% carbon 9.7 \% hydrogen and 51.6 \% oxygen. Its molar mass is 62.1 \mathrm{~g} \mathrm{~mol}^{-1} . Determine its empirical formula.?(Ans: \mathrm{CH}_{3} \mathrm{O} )
Q.16 Ethylene glycol is used as automobile antifreeze. It has 38.7 \% carbon 9.7 \% hydrogen and 51.6 \% oxygen. Its molar mass is 62.1 \mathrm{~g} \mathrm{~mol}^{-1} . Determine its empirical formula.?(Ans: \mathrm{CH}_{3} \mathrm{O} )

Q.16Ethyleneglycolisusedasautomobileantifreeze.Ithas38.7%carbon9.7%hydrogenand51.6%oxygen.Itsmolarmassis62.1 g mol−1.Determineitsempiricalformula.?(Ans:CH3O)Q.16 Ethylene glycol is used as automobile antifreeze. It has 38.7 \% carbon 9.7 \% hydrogen and 51.6 \% oxygen. Its molar mass is 62.1 \mathrm{~g} \mathrm{~mol}^{-1} . Determine its empirical formula.?(Ans: \mathrm{CH}_{3} \mathrm{O} )

Q.7 Boron with atomic number 5 has two naturally occurring isotopes. Calculate the percentage abundance of { }^{10} \mathrm{~B} and { }^{11} \mathrm{~B} from the following information.Average atomic mass of boron =10.81 \mathrm{amu} Isotopic mass of { }^{10} \mathrm{~B} =10.0129 \mathrm{amu} Isotopic mass of { }^{\prime \prime} \mathrm{B} =11.0093 \mathrm{amu} (Ans: 20.002 \% 79.992 \% )
Q.7 Boron with atomic number 5 has two naturally occurring isotopes. Calculate the percentage abundance of { }^{10} \mathrm{~B} and { }^{11} \mathrm{~B} from the following information.Average atomic mass of boron =10.81 \mathrm{amu} Isotopic mass of { }^{10} \mathrm{~B} =10.0129 \mathrm{amu} Isotopic mass of { }^{\prime \prime} \mathrm{B} =11.0093 \mathrm{amu} (Ans: 20.002 \% 79.992 \% )

Q.7Boronwithatomicnumber5hastwonaturallyoccurringisotopes.Calculatethepercentageabundanceof10 Band11 Bfromthefollowinginformation.Averageatomicmassofboron=10.81amuIsotopicmassof10 B=10.0129amuIsotopicmassof′′B=11.0093amu(Ans:20.002%79.992%)Q.7 Boron with atomic number 5 has two naturally occurring isotopes. Calculate the percentage abundance of { }^{10} \mathrm{~B} and { }^{11} \mathrm{~B} from the following information.Average atomic mass of boron =10.81 \mathrm{amu} Isotopic mass of { }^{10} \mathrm{~B} =10.0129 \mathrm{amu} Isotopic mass of { }^{\prime \prime} \mathrm{B} =11.0093 \mathrm{amu} (Ans: 20.002 \% 79.992 \% )

Q.5(a) What are isotopes? How do you deduce the fractional atomic masses of elements from the relative isotopic abundance? Give two examples in support of your answer.
Q.5(a) What are isotopes? How do you deduce the fractional atomic masses of elements from the relative isotopic abundance? Give two examples in support of your answer.

Q.5(a)Whatareisotopes?Howdoyoudeducethefractionalatomicmassesofelementsfromtherelativeisotopicabundance?Givetwoexamplesinsupportofyouranswer.Q.5(a) What are isotopes? How do you deduce the fractional atomic masses of elements from the relative isotopic abundance? Give two examples in support of your answer.

Q.25 Explain the following with reasons.i) Law of conservation of mass has to be obeyed during stoichiometric calculations.
Q.25 Explain the following with reasons.i) Law of conservation of mass has to be obeyed during stoichiometric calculations.

Q.25Explainthefollowingwithreasons.i)Lawofconservationofmasshastobeobeyedduringstoichiometriccalculations.Q.25 Explain the following with reasons.i) Law of conservation of mass has to be obeyed during stoichiometric calculations.

Calculate the number of grams of \mathrm{K}_{2} \mathrm{SO}_{4} and water produced when 14 \mathrm{~g} of \mathrm{KOH} are reacted with excess of \mathrm{H}_{2} \mathrm{SO}_{4} . Also calculate the number of molecules of water produced.
Calculate the number of grams of \mathrm{K}_{2} \mathrm{SO}_{4} and water produced when 14 \mathrm{~g} of \mathrm{KOH} are reacted with excess of \mathrm{H}_{2} \mathrm{SO}_{4} . Also calculate the number of molecules of water produced.

CalculatethenumberofgramsofK2SO4andwaterproducedwhen14 gofKOHarereactedwithexcessofH2SO4.Alsocalculatethenumberofmoleculesofwaterproduced.Calculate the number of grams of \mathrm{K}_{2} \mathrm{SO}_{4} and water produced when 14 \mathrm{~g} of \mathrm{KOH} are reacted with excess of \mathrm{H}_{2} \mathrm{SO}_{4} . Also calculate the number of molecules of water produced.

Define the following terms and give three examples of each.(i) Gram atom
Define the following terms and give three examples of each.(i) Gram atom

Definethefollowingtermsandgivethreeexamplesofeach.(i)GramatomDefine the following terms and give three examples of each.(i) Gram atom

banner6000+ MCQs with instant video solutions