XI Chemistry Stoichiometry Online Test Mdcat-2024

Instructions for Chapter Stoichiometry Online Test Mdcat-2024:

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Test Details:

Subject: Chemistry
Class: 1st year or 11
Chapter name: Stoichiometry
Test: MDCAT 2024
Book: Sindh Textbook
Total No. Of MCQS: 50
Time Allowed: 50 Minutes
Price : Free

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Created on June 10, 2024 By

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XI Chemistry Stoichiometry Online Test Mdcat-2024

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NameEmailPhone Number

1 / 50

1. The branch of Science, Which deals with the properties, composition, and structure of matter and also deals with change in matter and principles with govern these changes is called _________.

a) Bio-chemistry

b) Chemistry

c) Bioorganic chemistry

d) Physical chemistry

2 / 50

2. Atomic weight, formula and molecular weight in gram are called__.

a) Mass

b) Mole

c) Weight

d) None of these.

3 / 50

3. At S.T.P one mole of a substance occupies volume is 22.4 dm³. It is called ________.

a) Molal volume

b) Molar volume

c) Normal volume

d) Absolute volume

4 / 50

4. The Sum of atomic masses of element in a molecule is called _______.

a) Atomic mass

b) Molecular mass

c) Empirical formula

d) Mole

5 / 50

5. Stoichiometric calculations of a reaction give us yield called

a) Actual

b) Theoretical

c) Quantitative

d) None of these

6 / 50

6. The reactant that is consumed earlier & give least quantity of the product is called

a) Limiting reactant

b) Reactant

c) Stoichiometry

d) none of these

7 / 50

7. The amount of product obtained or calculated from balanced chemical equation is

called:

a) Actual yield

b) Theoretical yield

c) Experimental yield

d) Balanced yield

8 / 50

8. 8.46gm of Na metal contains

a) 3.01 x 10²³atoms

b) 6.02 x 10²³atoms

c) 12.04 x 10²³atoms

d) None of these

9 / 50

9. The volume occupied by 1.4gm of N₂ at S.T.P is

a) 2.24dm³

b) 22.4 dm³

c) 11.2dm³

d) 1.12dm³

10 / 50

10.

3.01 x 10²³molecules of H₂O will weight

a) 18gm

b) 9gm

c) 4.5gm

d) None of these

11 / 50

11. The number of molecules in 28 grams of Nitrogen are:

a) 6.02 × 10²³

b) 12.04 × 10²³

c) 3.01 × 10²³

d) 1.204 × 10²³

12 / 50

12. At STP, 22.4 dm³ of CO₂ ____________ 22.4 dm³ of SO₂:

a) Heavier than

b) Lighter than

c) Equal to

d) Double

13 / 50

13. The number of moles present 100 grams of water are:

a) 5.56

b) 27.78

c) 6.25

d) 0.18

14 / 50

14. Molecular weight is used for the substances which are:

a) Ionic

b) Non-Ionic

c) Neutral

d) Atomic Molecules

15 / 50

15. The number of particles present in one mole are:

a) 6.02 × 10²¹

b) 6.02 × 10²²

c) 6.02 × 10²³

d) 6.02 × 10²⁴

16 / 50

16. Atomic weight is the average weight of atoms of an element as compared to the weight

of one atom of carbon taken as:

a) 12

b) 13

c) 14

d) 15

17 / 50

17. 58.5 amu of NaCl is:

a) Atomic Weight

b) Formula Weight

c) Molecular Weight

d) Ionic Weight

18 / 50

18. 18.0 amu of water is:

a) Atomic Weight

b) Formula Weight

c) Molecular Weight

d) Ionic Weight

19 / 50

19. Very small and very large quantities are expressed in terms of:

a) Significant figures

b) Exponential notation

c) Logarithm

d) All of these

20 / 50

20. Number of molecules in two moles of water are:

a) 6.02 × 10²³

b) 1.204 × 10²⁴

c) 3.01 × 10²³

d) 12.04 × 10²⁴

21 / 50

21. A reaction is known to have a percent yield of 80%. It the actual yield is 25 grams, what was the expected yield?

a) 25 g

b) 31.25g

c) 35 g

d) 19.5 g

22 / 50

22. 12.044 x 10²³ atoms of oxygen contains ___________

a) 1 mole of oxygen

b) 2 moles of oxygen

c) 3 moles of oxygen

d) 4 moles of oxygen

23 / 50

23. The mass of 0.3 moles of ammonia is

a) 21g

b) 5.1g

c) 17g

d) 2.1 g

24 / 50

24. The volume occupied by 1.5 mole of glucose will be

a) 22.4 dm³

b) 11.2 dm³

c) 33.6 dm³

d) 44.8 m³

25 / 50

25. The amount of carbon dioxide produced by the combustion of 40g of methane is.

CH₄ +2O₂→CO₂+2H₂O

a) 44g

b) 110g

c) 66g

d) 22g

26 / 50

26. The number 75.66852 rounded off to 5 significant digits is

a) 75.67

b) 75.669

c) 75.668

d) 75.667

27 / 50

27. When 4 moles of propane react with 6 moles of oxygen, the mass of CO2 produced will be

C₃H₈ + 5O₂ →3CO₂ + 4H₂O

a) 180 g

b) 158.4 g

c) 460 g

d) 350 g

28 / 50

28. Which of the following does not represent a chemical change?

a) Burning of leaves

b) Fermentation of grapes

c) Turning brown of freshly cut banana

d) Freezing of water

29 / 50

29. Which of the following is incorrect for a chemical reaction?

a) Heat is released only but never absorbed

b) change in composition occurs

c) A colour change may take place

d) A gas may be evolved

30 / 50

30. The most abundant element in the universe is

a) Hydrogen

b) Oxygen

c) Carbon dioxide

d) Silicon

31 / 50

31. The formula weight of the compound, Al₂ (SO₄)₃.18H₂O is:

a) 394 g

b) 666 g

c) 693 g

d) 466 g

32 / 50

32. How many moles of alanine, C₃H₇NO₂, are there in 159 g of alanine?

a) 1.42

b) 1.78

c) 9.92

d) 5.60

33 / 50

33. How many atoms are in one mole of methanol (CH₃OH)?

a) 6.02 x10²³

b) 6.0 x 10²³

c) 12.0 x 10²³

d) 3.6 x 10²⁴

34 / 50

34. The mass in grams of 3.01 x 10²³ calcium atom is:

a) 44

b) 11.5

c) 20

d) 1.5

35 / 50

35. Which one of the samples contains the large number of atoms?

a) 1 mol of CO₂

b) 1 mol of C₆H₁₂O₆

c) 1 mol of CH₃COCH₃

d) 1 mol of CH₄

36 / 50

36. The percent by mass of nitrogen in given fertilizer is HNC (NH₂)₂

a) 45.2%

b) 49.4%

c) 54.8%

d) 71.1%

37 / 50

37. The amount of water produced when 8g of hydrogen is reacted with 32g of oxygen is

2H₂+O₂ 2H₂O

a) 2moles

b) 1mole

c) 3 moles

d) 0.5mole

38 / 50

38. What volume of hydrogen at RTP would be liberated, when 8 gm of calcium reacts with excess water?

Ca + 2H₂O Ca(OH)₂ + H₂

a) 44.80 dm³

b) 22.4 dm³

c) 4.88 dm³

d) 0.4 dm³

The balanced chemical equation for the reaction is:

Ca + 2H₂O → Ca(OH)₂ + H₂

Step 1: Calculate the Moles of Calcium

The molar mass of calcium (Ca) is 40 g/mol.

Moles of calcium in 8 grams:

Moles of Ca = 8 g / 40 g/mol = 0.2 moles

Step 2: Determine the Moles of Hydrogen Gas Produced

From the balanced equation, 1 mole of calcium produces 1 mole of hydrogen gas (H₂).

Therefore, 0.2 moles of calcium will produce 0.2 moles of hydrogen gas.

Step 3: Calculate the Volume of Hydrogen Gas at RTP

At RTP (Room Temperature and Pressure), 1 mole of any gas occupies 24 liters.

The volume of 0.2 moles of H₂:

Volume of H₂ = 0.2 moles × 24 L/mole = 4.8 liters

Conclusion

The volume of hydrogen gas liberated when 8 grams of calcium reacts with excess water is 4.8 liters.

39 / 50

39. The number of molecules in 2.5 moles of H2O?

a) 6.023 x 10¹⁹

b) 6.023 x 10²³

c) 1.505 x 10²⁴

d) 1.20 x10²⁴

40 / 50

40. A necklace has 12 g of diamond in it. What are the number of atoms in it?

a) 6.02 x 10²³

b) 12.04 x 10²³

c) 1.003 x 10²³

d) 3.01 x 10²³

41 / 50

41. The branch of Chemistry which deals with the calculations based on balanced chemical

equations is called

a) Environmental Chemistry

b) Physical Chemistry

c) Stoichiometry

d) Industrial Chemistry

42 / 50

42. If one mole of each of the following substance is burnt in oxygen completely, which will give the largest volume of CO₂?

a) Graphite

b) Diamond

c) Ethane

d) Methane

43 / 50

43. The Avogadro's constant is the number of?

a) Atoms in 1 g of Helium

b) Molecules in 35.5 g of chloride

c) Molecules in 23 g of Na

d) Atoms in 24 g of Mg

44 / 50

44. A limiting reactant is that which

a) Is taken in lesser quantity in grams as compared to other reactants

b) Is taken in lesser quantity in volume as compared to other reactants

c) Gives the maximum amount of the product

d) Gives the minimum amount of the product.

45 / 50

45. Which among the following is the heaviest?

a) One mole of oxygen

b) One molecule of Sulphur trioxide

c) 50 atoms of Aluminum

d) 44g of Carbon dioxide

46 / 50

46. Theoretical yield is always less than the actual yield because:

a) Some product is lost in the experiment

b) Reversible reaction may occur

c) Errors are made in weighing the reactants or the products

d) None of these.

47 / 50

47. Stoichiometry is ………………. analysis of the calculations during a chemical reaction.

a) Quantitative

b) Qualitative

c) volumetric

d) none of these

48 / 50

48. If the reaction of 6.5 grams of C₆H₁₂O₆ produces 2.5 grams of CO₂, what is the percent yield of CO2?

C₆H₁₂O₆-------> 2C₂H₅OH + 2CO₂

a) 78.86%

b) 90%

c) 92%

d) 92.25%

49 / 50

49. After a reaction was run, there were 12.7 grams of reagent B left over. Reagent B is the

a) Superfluous reagent

b) Excess reagent

c) Extra reagent

d) limiting reagent

50 / 50

50. Percent yield is found by

a) Theoretical Yield / Actual Yield x 100 percent

b) Actual Yield x Theoretical Yield x 100 percent

c) Actual Yield / Theoretical Yield x 100 percent

d) All of the above

Your score is

Instructions for Chapter Stoichiometry Online Test Mdcat-2024:

Test Details:

Step 1: Calculate the Moles of Calcium

Step 2: Determine the Moles of Hydrogen Gas Produced

Step 3: Calculate the Volume of Hydrogen Gas at RTP

Conclusion

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