Fundamentals Of Chem Flashcards
(50 cards)
1
Q
- Empirical formula of formaldehyde HCHO is same with (A) Acetaldehyde (B) Ethanol (C) Glucose (D) All of these
A
(C) Glucose
2
Q
- During combustion analysis KOH is used to absorb (A) Oxygen gas (B) Hydrogen gas (C) H₂O vapours (D) CO₂
A
(D) CO₂
3
Q
- Out of 280 isotopes how many isotopes have even atomic no and even mass no (A) 152 (B) 153 (C) 154 (D) 155
A
(C) 154
4
Q
- The largest number of molecules are present in (A) 0.4H₂ (B) 3.2gO₂ (C) 2.8g N₂ (D) 18g glucose
A
(A) 0.4H₂
5
Q
- A mole of ozone gas contains ______ no of atoms (A) 6.02×10²³ (B) 12.04×10²³ (C) 18.06×10²³ (D) 1.05×10²³
A
(C) 18.06×10²³
6
Q
- The molecules of hemoglobin is ______ heavier than H-atom (A) 67000 times (B) 68000 times (C) 65000 times (D) 69000 times
A
(B) 68000 times
7
Q
- Which of the following has eleven isotopes (A) Palladium (B) Tin (C) Cadmium (D) Calcium
A
(B) Tin
8
Q
- No of covalent bonds in 18g of H₂O (A) 6.02×10²³ (B) 12.04×10²³ (C) 18.06×10²³ (D) 1.05×10²³
A
(B) 12.04×10²³
9
Q
- 96g SO₄²⁻ and 62g NO₃⁻ have number of ions (A) Same (B) Different (C) SO₄²⁻ has more (D) NO₃⁻ has more
A
(A) Same
10
Q
- Limiting reactant control the amount of ______ (A) Reactant (B) Product (C) Both A & B (D) None of these
A
(B) Product
11
Q
- Total no of electron present in 46g Na⁺ are (A) 23Na (B) 2Na (C) 20Na (D) 10Na
A
(C) 20Na
12
Q
- The relative abundance of isotopes of elements is measured by (A) Atomic spectroscopy (B) Ionic spectroscopy (C) Mass spectroscopy (D) Mass of spectrometry
A
(C) Mass spectroscopy
13
Q
- Number of molecules in 1dm³ of water will be almost (A) 18×6.02×10²³ (B) 55.6×6.02×10²³ (C) 6.02×10²³ (D) 2×6.02×10²³
A
(B) 55.6×6.02×10²³
14
Q
- The relative mass of copper is (A) 63.345 amu (B) 63.455 amu (C) 63.546 amu (D) 63.65 amu
A
(C) 63.546 amu
15
Q
- Isotopes are the atoms of same element having different number of (A) Electron (B) Proton (C) Positron (D) Neutron only
A
(D) Neutron only
16
Q
- The phenomenon of isotropy was first discovered by (A) Dalton’s (B) Soddy (C) J. Perrin (D) J. Berzelius
A
(B) Soddy
17
Q
- According to Dalton’s atomic theory all the atoms of an element (A) Different in size (B) Different in mass number (C) Were considered alike in their mass (D) All of these
A
(C) Were considered alike in their mass
18
Q
- Which set of elements have three isotopes (A) O H (B) O Cl (C) Cl Hg (D) All of these
A
(A) O H
19
Q
- The ozone is isotope of (A) O (B) H (C) Cl (D) None of these
A
(D) None of these
20
Q
- 9.8g of phosphoric acid dissolved in excess quantity of water it will yield ______ moles of hydrogen ion (H⁺) ______ moles of phosphate (PO₄³⁻) (A) 0.1 0.2 (B) 0.1 0.3 (C) 0.2 0.1 (D) 0.3 0.1
A
(D) 0.3 0.1
21
Q
- The mass of one mole of electron is (A) 1.00mg (B) 0.55mg (C) 0.184mg (D) 1.673mg
A
(B) 0.55mg
22
Q
- ______ of Al will react completely with 48g O₂ to produce Al₂O₃ (A) 27g (B) 24g (C) 54g (D) 67g
A
(C) 54g
23
Q
- The no of moles of NO₂ which contains 16g of oxygen (A) 0.25 (B) 0.50 (C) 1.0 (D) 1.50
A
(B) 0.50
24
Q
- One mole of water contains I) 6.02×10²³ atoms of hydrogen II) 1gram molecules of H₂O IV) Molecules having 22.4dm³ value (A) I and III (B) II and III (C) II III and IV (D) I III and IV
A
(B) II and III
25
25. 90g of glucose contains ______ atoms of carbon (A) 0.5NA (B) 3NA (C) 6NA (D) 12NA
(B) 3NA
26
26. The number of atoms in 1.97g gold and 0.023g of sodium are (A) Equal (B) Different (C) Sodium contains more atoms than gold (D) None of these
(B) Different
27
27. One mg of K₂CrO₄ has ______ the number of ions than the number of formula units when dissolved in water (A) Twice (B) Thrice (C) Same (D) None of these
(A) Twice
28
28. Two grams of H₂ 16g CH₄ occupy separately the volume of 22.414dm³ (A) Size of molecules of two gases are same (B) Masses of molecules two gases are same (C) Number of molecules of two gases are same (D) All of these
(C) Number of molecules of two gases are same
29
29. A sample of 0.600 mol of a metal calcium reacts completely with excess of fluorine to calcium fluoride how many moles of F are present in calcium fluoride (A) 0.6 (B) 0.3 (C) 1.2 (D) 1.8
(C) 1.2
30
30. 0.4 moles of ozone and 0.4 moles of oxygen gas have (A) Different no of molecules (B) Same no of atoms (C) Different no of atoms (D) Different volume at STP
(C) Different no of atoms
31
31. Which contain more % of nitrogen (A) NH₃ (B) NH₂CONH₂ (C) (NH₄)₂SO₄ (D) NH₄NO₃
(A) NH₃
32
32. 22.4dm³ of CO and 22.4dm³ N₂ have the same no of (A) Electron (B) Protons (C) Neutrons (D) All of these
(D) All of these
33
33. One mole of H₂SO₄ reacts with two moles of NaOH How many molecules of water are produced (A) 6.02×10²³ (B) 12.04×10²³ (C) 18.06×10²³ (D) 24.08×10²³
(A) 6.02×10²³
34
34. How many moles of N₂ are produced when 1 mole of N₂O₄ react with 1 mole of N₂H₄ 2N₂H₄ + N₂O₄ → 3N₂ + 4H₂O (A) 3 (B) 2 (C) 1.5 (D) 1
(C) 1.5
35
35. The volume occupied by 1.4g CO (A) 2.24dm³ (B) 22.4dm³ (C) 1.12dm³ (D) 112cm³
(C) 1.12dm³
36
36. No of formula units in 58.5g NaCl (A) 6.02×10²³ (B) 12.04×10²³ (C) 18.06×10²³ (D) One
(A) 6.02×10²³
37
37. The amount of the products calculated from the balanced chemical equation represent the (A) Actual yield (B) Theoretical yield (C) % yield (D) None of these
(B) Theoretical yield
38
38. The efficiency of a reaction is expressed in the form of (A) Practical yield (B) Theoretical yield (C) Percentage % yield (D) None of these
(C) Percentage % yield
39
39. How many moles of H₂O will produce when 2moles of H₂ combine with 2 moles of O₂ (A) 1 mole (B) 2 mole (C) 3 mole (D) 4 mole
(B) 2 mole
40
40. How many moles of HCl are required to produce 12 moles of H₂ according to the equation Mg(s) + 2HCl(aq) → MgCl(aq) + H₂(g) (A) 12 mole (B) 6 mole (C) 24 mole (D) 48 mole
(C) 24 mole
41
41. The branch of chemistry which tells us the quantative relationship b/w reactant and product in a balanced chemical equation (A) Mass – mass relationship (B) Limiting reactant (C) Stoichiometry (D) Thermo chemistry
(C) Stoichiometry
42
42. In gaseous state the distance b/w molecules is ______ times greater than their diameter (A) 2 (B) 3 (C) 4 (D) 300
(D) 300
43
43. One mole of any gas at room temperature and pressure occupies (A) 22.414dm³ (B) 24dm³ (C) 1dm³ (D) 10dm³
(B) 24dm³
44
44. Mass of 0.1 mole of PO₄³⁻ ion (A) 95g (B) 9.5g (C) 0.95g (D) 0.98g
(B) 9.5g
45
45. How many molecules of water are there in 10g of Ice (A) 3.01×10²³ molecules (B) 2.408×10²³ molecules (C) 6.02×10²³ molecules (D) 3.31×10²³ molecules
(A) 3.01×10²³ molecules
46
46. No of gram ions in 1.7g OH⁻ (A) 6.02×10²² (B) 1 (C) 0.1 (D) 0.01
(C) 0.1
47
47. No of moles in 0.28kg of silicon (A) 0.1 (B) 0.01 (C) 1 (D) 10
(D) 10
48
48. No of gram atoms of hydrogen in 2.016g of hydrogen (A) 1 (B) 2 (C) 12.04×10²³ (D) 6.02×10²³
(B) 2
49
49. Which of the following compounds have same empirical and molecular formula (A) C₆H₂O₆ (B) C₁₂H₂₂O₁₁ (C) C₂H₄O₂ (D) All of these
(C) C₂H₄O₂
50
50. Which of the following is mono isotopic element (A) Iodine (B) Chlorine (C) Bromine (D) All of these
(A) Iodine
