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Question 1 of 100
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Question 1

What is the molarity of a solution containing 4.74 moles of solute in 2.0 L of solution?

Question 2

What is the molarity of a solution containing 2.09 moles of solute in 2.0 L of solution?

Question 3

What is the molarity of a solution containing 4.39 moles of solute in 0.25 L of solution?

Question 4

What is the molarity of a solution containing 4.49 moles of solute in 2.0 L of solution?

Question 5

What is the molarity of a solution containing 2.41 moles of solute in 2.0 L of solution?

Question 6

What is the molarity of a solution containing 0.61 moles of solute in 5.0 L of solution?

Question 7

What is the molarity of a solution containing 1.86 moles of solute in 1.0 L of solution?

Question 8

What is the molarity of a solution containing 0.18 moles of solute in 1.0 L of solution?

Question 9

What is the molarity of a solution containing 4.0 moles of solute in 2.0 L of solution?

Question 10

What is the molarity of a solution containing 4.83 moles of solute in 2.0 L of solution?

Question 11

What is the molarity of a solution containing 1.28 moles of solute in 0.5 L of solution?

Question 12

What is the molarity of a solution containing 1.54 moles of solute in 0.25 L of solution?

Question 13

What is the molarity of a solution containing 2.72 moles of solute in 5.0 L of solution?

Question 14

What is the molarity of a solution containing 0.22 moles of solute in 1.0 L of solution?

Question 15

What is the molarity of a solution containing 3.55 moles of solute in 0.25 L of solution?

Question 16

Calculate the molality of a solution where 1.42 moles of solute are dissolved in 2500.0 g of solvent.

Question 17

Calculate the molality of a solution where 1.72 moles of solute are dissolved in 100.0 g of solvent.

Question 18

Calculate the molality of a solution where 2.79 moles of solute are dissolved in 2000.0 g of solvent.

Question 19

Calculate the molality of a solution where 0.85 moles of solute are dissolved in 100.0 g of solvent.

Question 20

Calculate the molality of a solution where 2.02 moles of solute are dissolved in 2500.0 g of solvent.

Question 21

Calculate the molality of a solution where 0.11 moles of solute are dissolved in 2000.0 g of solvent.

Question 22

Calculate the molality of a solution where 2.46 moles of solute are dissolved in 500.0 g of solvent.

Question 23

Calculate the molality of a solution where 2.44 moles of solute are dissolved in 2500.0 g of solvent.

Question 24

Calculate the molality of a solution where 2.36 moles of solute are dissolved in 500.0 g of solvent.

Question 25

Calculate the molality of a solution where 0.94 moles of solute are dissolved in 100.0 g of solvent.

Question 26

Calculate the molality of a solution where 1.85 moles of solute are dissolved in 100.0 g of solvent.

Question 27

Calculate the molality of a solution where 0.2 moles of solute are dissolved in 500.0 g of solvent.

Question 28

Calculate the molality of a solution where 0.92 moles of solute are dissolved in 2500.0 g of solvent.

Question 29

Calculate the molality of a solution where 1.88 moles of solute are dissolved in 500.0 g of solvent.

Question 30

Calculate the molality of a solution where 1.29 moles of solute are dissolved in 2000.0 g of solvent.

Question 31

How many molecules are present in 0.5 moles of a substance?

Question 32

How many molecules are present in 0.1 moles of a substance?

Question 33

How many molecules are present in 5 moles of a substance?

Question 34

How many molecules are present in 2 moles of a substance?

Question 35

How many molecules are present in 0.5 moles of a substance?

Question 36

How many molecules are present in 0.5 moles of a substance?

Question 37

How many molecules are present in 5 moles of a substance?

Question 38

How many molecules are present in 0.5 moles of a substance?

Question 39

How many molecules are present in 1 moles of a substance?

Question 40

How many molecules are present in 3 moles of a substance?

Question 41

How many molecules are present in 0.1 moles of a substance?

Question 42

How many molecules are present in 2 moles of a substance?

Question 43

How many molecules are present in 0.1 moles of a substance?

Question 44

How many molecules are present in 0.1 moles of a substance?

Question 45

How many molecules are present in 3 moles of a substance?

Question 46

What is the volume occupied by 0.5 moles of an ideal gas at STP?

Question 47

What is the volume occupied by 2 moles of an ideal gas at STP?

Question 48

What is the volume occupied by 0.5 moles of an ideal gas at STP?

Question 49

What is the volume occupied by 2 moles of an ideal gas at STP?

Question 50

What is the volume occupied by 1 moles of an ideal gas at STP?

Question 51

What is the volume occupied by 0.5 moles of an ideal gas at STP?

Question 52

What is the volume occupied by 1 moles of an ideal gas at STP?

Question 53

What is the volume occupied by 2 moles of an ideal gas at STP?

Question 54

What is the volume occupied by 0.1 moles of an ideal gas at STP?

Question 55

What is the volume occupied by 2 moles of an ideal gas at STP?

Question 56

What is the volume occupied by 2 moles of an ideal gas at STP?

Question 57

What is the volume occupied by 0.5 moles of an ideal gas at STP?

Question 58

What is the volume occupied by 2 moles of an ideal gas at STP?

Question 59

What is the volume occupied by 0.5 moles of an ideal gas at STP?

Question 60

What is the volume occupied by 0.25 moles of an ideal gas at STP?

Question 61

A compound has the molecular formula C5H10. What is its empirical formula?

Question 62

A compound has the molecular formula C2H4. What is its empirical formula?

Question 63

A compound has the molecular formula C6H12. What is its empirical formula?

Question 64

A compound has the molecular formula C6H12. What is its empirical formula?

Question 65

A compound has the molecular formula C6H12. What is its empirical formula?

Question 66

A compound has the molecular formula C4H8. What is its empirical formula?

Question 67

A compound has the molecular formula C2H4. What is its empirical formula?

Question 68

A compound has the molecular formula C6H12. What is its empirical formula?

Question 69

A compound has the molecular formula C2H4. What is its empirical formula?

Question 70

A compound has the molecular formula C3H6. What is its empirical formula?

Question 71

How many significant figures are in the number 100.0?

Question 72

How many significant figures are in the number 100.0?

Question 73

How many significant figures are in the number 1.005?

Question 74

How many significant figures are in the number 0.0050?

Question 75

How many significant figures are in the number 0.05?

Question 76

How many significant figures are in the number 100?

Question 77

How many significant figures are in the number 0.0050?

Question 78

How many significant figures are in the number 100?

Question 79

How many significant figures are in the number 100.0?

Question 80

How many significant figures are in the number 100.0?

Question 81

How many significant figures are in the number 100?

Question 82

How many significant figures are in the number 100.0?

Question 83

How many significant figures are in the number 0.05?

Question 84

How many significant figures are in the number 100.0?

Question 85

How many significant figures are in the number 100.0?

Question 86

What is the molar mass of Water (H2O)?

Question 87

What is the molar mass of Carbon dioxide (CO2)?

Question 88

What is the molar mass of Methane (CH4)?

Question 89

What is the molar mass of Ammonia (NH3)?

Question 90

What is the molar mass of Sodium chloride (NaCl)?

Question 91

How many moles are in 54 g of Water (H2O)?

Question 92

How many moles are in 88 g of Carbon dioxide (CO2)?

Question 93

How many moles are in 32 g of Methane (CH4)?

Question 94

How many moles are in 51 g of Ammonia (NH3)?

Question 95

How many moles are in 117.0 g of Sodium chloride (NaCl)?

Question 96

What is the SI unit of amount of substance?

Question 97

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

Question 98

The sum of the atomic masses of all atoms in a molecule is known as:

Question 99

Law of multiple proportions was proposed by:

Question 100

One atomic mass unit (amu) is equivalent to: