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Chemistry Essentials Quiz

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Chemistry Essentials Quiz

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Core topics recap

Created by

Owen Blankenfeld
Owen Blankenfeld
United States

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Chemistry Essentials Quiz
 

Chemistry Essentials QuizOnline version

Core topics recap

by Owen Blankenfeld
1

How many significant figures are in 0.02050 g?

2

How many significant figures are in 120 mL?

3

What conversion factor is used to convert 0.750 liters to milliliters?

4

Why is density considered an intensive property?

5

A student measures 25.0 mL, 25.1 mL, and 24.9 mL. The true value is 30.0 mL. Are the measurements accurate and/or precise?

6

What is (2.50 × 10^2) × (4.00 × 10^-5)?

7

A student calculates copper’s density as 8.42 g/cm^3. The accepted value is 8.96 g/cm^3. What is the percent error?

8

An object has mass 26.5 g and displaces water from 15.0 mL to 21.0 mL. What is its density?

9

According to the Law of Conservation of Mass, if 24.3 g Mg reacts with 16.0 g O, what is mass of MgO produced?

Feedback

Significant figures are the digits that carry meaning in a measurement; trailing zeros after decimal are significant.

Without a decimal point, trailing zeros may not indicate precision.

There are 1000 mL in 1 L.

Intensive properties do not depend on sample size.

Values are close to each other (precise) but far from the true value (not accurate).

Multiply coefficients: 2.50×4.00=10.00; powers add to 2-5 = -3; result 1.00×10^-2.

Percent error = |experimental - accepted| / accepted × 100%.

Density = mass / volume; volume = 21.0-15.0 = 6.0 mL.

Mass is conserved in chemical reactions.

 
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