If you are searching for the important short questions of 11th class physics then here we have shared the 1st Year Physics Important Short Questions Chapter 1
2) One mg of K2CrO4 has thrice the number of ions then the number of formula units when ionized in water. Justify.
3) How many numbers of molecules in 10g of ice?
4) Why theoretical yield is always larger than the actual yield?
5) What is the mass spectrum?
6) Define empirical formula and the molecular formula with examples? Explain the relation between them?
7) N2 and CO have the same number of electrons, protons, and neutrons?
8) Define the term molecule and give two examples?
9) No individual neon atom in the sample of the element has a mass of 20.18amu. Explain?
10) Define stoichiometry and explain its assumptions?
11) Calculate the mass in kg of 2.0 × 1020 molecules of SO2?
12) Write functions of Mg(ClO4)2 and KOH in combustion analysis?
13) Why we calculate %age yield?
14) Mg atom is twice heavier than C atom. Justify?
15) A compound may have the same empirical formula as well as the molecular formula. Justify?
16) What is Avogadro’s number? Give its relation with the mass of an element?
17) What are isotopes? Why they have the same chemical properties and different physical properties?
18) Differentiate between ion and molecular ion?
19) Calculate the mass in grams of 10-3 moles of water?
20) Calculate the moles of O atoms in 9.00 g of Mg(NO3)2.
21) One mole of H2SO4 should completely react with two moles of NaOH. How does Avogadro’s number help to explain it?
22) Describe that one mole of H2O has two moles of the bond, three moles of atoms, ten moles of electrons and twenty-eight moles of the total fundamental particles present in it?
23) Why chemical reaction taking place in our surroundings involve the limiting reactants?
24) What is the function of the electric field in mass spectrometer?
25) Why 23g of Na and 238g of uranium have an equal number of atoms in them?
26) Why 2g of H2, 16g of CH4 and 44g of CO2 occupy separately the volume of 22.414dm3 although the sizes of masses molecules of these three gases are very different from each other?
27)Calculate mass In grams of 2.74 moles of KMnO4. The formula mass of KMnO4 is 158gmol-1?
Chapter 1 SHORT QUESTIONS:
1) The Law of conservation of mass has to be obeyed during stoichiometry calculations. Give a reason?2) One mg of K2CrO4 has thrice the number of ions then the number of formula units when ionized in water. Justify.
3) How many numbers of molecules in 10g of ice?
4) Why theoretical yield is always larger than the actual yield?
5) What is the mass spectrum?
6) Define empirical formula and the molecular formula with examples? Explain the relation between them?
7) N2 and CO have the same number of electrons, protons, and neutrons?
8) Define the term molecule and give two examples?
9) No individual neon atom in the sample of the element has a mass of 20.18amu. Explain?
10) Define stoichiometry and explain its assumptions?
11) Calculate the mass in kg of 2.0 × 1020 molecules of SO2?
12) Write functions of Mg(ClO4)2 and KOH in combustion analysis?
13) Why we calculate %age yield?
14) Mg atom is twice heavier than C atom. Justify?
15) A compound may have the same empirical formula as well as the molecular formula. Justify?
16) What is Avogadro’s number? Give its relation with the mass of an element?
17) What are isotopes? Why they have the same chemical properties and different physical properties?
18) Differentiate between ion and molecular ion?
19) Calculate the mass in grams of 10-3 moles of water?
20) Calculate the moles of O atoms in 9.00 g of Mg(NO3)2.
21) One mole of H2SO4 should completely react with two moles of NaOH. How does Avogadro’s number help to explain it?
22) Describe that one mole of H2O has two moles of the bond, three moles of atoms, ten moles of electrons and twenty-eight moles of the total fundamental particles present in it?
23) Why chemical reaction taking place in our surroundings involve the limiting reactants?
24) What is the function of the electric field in mass spectrometer?
25) Why 23g of Na and 238g of uranium have an equal number of atoms in them?
26) Why 2g of H2, 16g of CH4 and 44g of CO2 occupy separately the volume of 22.414dm3 although the sizes of masses molecules of these three gases are very different from each other?
27)Calculate mass In grams of 2.74 moles of KMnO4. The formula mass of KMnO4 is 158gmol-1?
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