Free Printable quiz 7 (sec. 1)

1.

What is the concentration percentage of a solution of sucrose C₁₂H₂₂O₁₁ whose one liter contains one mole of the solute? [C= 12, H=1, O=16]

a)

6.84%

b)

10%

c)

34.2%

d)

100%

2.

Which of the following solutions contains higher number of moles of the solute?

a)

10 mL of 0.5 mol/L NaCl solution.

b)

20 mL of 0.4 mol/L NaCl solution.

c)

30 mL of 0.3 mol/L. NaCI solution.

d)

40 mL of 0.2 mol/L NaCl solution.

3.

The mass of sodium carbonate which is required to prepare 500 mL of 0.5 M solution equals ............... [Na=23, C=12, O=16]

a)

10000 g

b)

106 g

c)

40 g

d)

26.5 g

4.

The concentration percentage of a molar solution of sulphuric acid H₂SO₄ equals ....... [H=1, S=32, O=16]

a)

0.098%

b)

0.98%

c)

9.8%

d)

98%

5.

What is the concentration of sulphuric acid which 25 mL of it react completely with 36.2 mL of 0.225 M sodium hydroxide solution?

a)

$\frac{36.2\times0.225}{25}M$

b)

$\frac{2\times36.2\times0.225}{25}M$

c)

$36.2\times\frac{0.225}{2\times25}M$

d)

$\frac{25}{2\times36.2\times0.225}M$

6.

What is the volume of water which is required to be added to 328 g of NaOH to form a solution whose concentration is 1.35m? [Na=23, O=16, H=1]

a)

6.07 L

b)

7.44

c)

11.1 L

d)

14.5 L

7.

A sugar solution was made by mixing 12 g of glucose with 100 g of water. What is the percentage concentration by mass of the glucose in the solution? Give your answer to one decimal place.

a)

12.0%(m/m)

b)

11.4%(m/m)

c)

13.6%(m/m)

d)

10.7%(m/m)

8.

Which of the following equations can be used to calculate the percentage by volume, %(v/v), of a solution?

a)

% (V/V)= $\left(\frac{volume\ of\ solution\ }{volume\ of\ solute\ }\right)\times100\%$

b)

% (V/V)= $\left(\frac{volume\ of\ solute\times volume\ of\ solution}{100\%}\right)$

c)

% (V/V)= $\left(\frac{100\%}{volume\ of\ solute\ \times volume\ of\ solution\ }\right)$

d)

% (V/V)= $\left(\frac{volume\ of\ solute\ }{volume\ of\ solution\ }\right)\times100\%$

9.

Which of the following statements best describes the concentration of a solution?

a)

How reactive a solute is with water

b)

The amount of solvent dissolved in a certain volume of solute

c)

The amount of solute dissolved in a certain volume of solution

d)

How quickly a solute dissolves in a solvent

10.

By dissolving 25 mL of oil in an amount of benzene, a solution of 40% percentage concentration (v/v) is obtained. Calculate the volume of benzene used to prepare the solution. Give your answer to one decimal place.

a)

62.5 mL

b)

65.0 mL

c)

87.5 mL

d)

37.5 mL

11.

Which of the following explains why a reaction yield may appear to be above 100%?

a)

There are two or more reactions that occur simultaneously so that some reactants are converted to products

b)

All reactions are complete; therefore, all reactants are converted to products.

c)

The reagents are of high purity.

d)

The product of the reaction contains impurities

12.

The combustion of methanol can be represented by the following chemical equation:

2CH₃OH + 3O₂ = CO₂ + 4H₂O

In which of the following molar ratios, between CH₃OH and O₂, will there be an excess of oxygen?

a)

5∶3

b)

1∶3

c)

4∶6

d)

2∶1

13.

What is the formula for calculating the percentage yield from the actual yield and the theoretical yield?

a)

Percentage yield = actual yield / theoretical yield

b)

Percentage yield = (theoretical yield / actual yield) × 100%

c)

Percentage yield = theoretical yield / actual yield

d)

Percentage yield = (actual yield / theoretical yield) × 100%

14.

29 g of butane gas C₄H₁₀ are burnt in excess of oxygen gas forming 0.9g of water vapor H₂O, what is the percentage of the actual yield of water vapor?

a)

0.002%

b)

2%

c)

10%

d)

36%

15.

What is the mass percentage of iron in iron (III) oxide?

a)

0.72%

b)

28%

c)

30%

d)

69.9%

16.

According to Avogadro’s law, what happens to the volume a gas occupies if the number of moles increases?

a)

It stays the same.

b)

It increases.

c)

It decreases.

d)

none of them

17.

A 65 kg woman has 8.9×10^-3 mol of hemoglobin (molar mass = 64‎ ‎456 g/mol) in her blood.

How many hemoglobin molecules are there?

a)

5.4×10²¹

b)

5.4×10¹⁹

c)

5.4×10²³

d)

5.4×10²²

18.

What is the mass of 0.25 L (at STP) of the gas (X) whose molar mass = 62.7 g/mol?

a)

0.69 g

b)

0.35 g

c)

0.07 g

d)

0.035 g

19.

What is the number of molecules in a sample of ammonia NH₃ its mass equals 43.5 g? ________ Molecules?

a)

2.62 x 10²⁵

b)

1.54x 10²⁴

c)

2.36 x 10²³

d)

8.63 x 10^-16

20.

What is the molar mass of barium sulphite? [Ba = 137, S=32, O= 16]

a)

514 g/mol

b)

233 g/mol

c)

354 g/mol

d)

217 g/mol

quiz 7 (sec. 1)

Total questions: 20

Worksheet time: 2hrs 40mins

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