Question 1

A student determined the mass of a sample contained in a beaker by subtracting the mass of the beaker alone ($73.8 \ \mathrm{g}$) from the mass of the beaker containing the sample ($75.652 \ \mathrm{g}$). How many significant figures should be reported for the mass of the sample?

Accepted Answer

2 significant figures

Question 2

Which of the following calculations is performed correctly according to the rules for significant figures? $12.32 - 12.22 \div 3.97$

Accepted Answer

$0.025$

Question 3

Given the calculation $98.00725084 + 2.8053281$, how many significant figures should the answer have?

Accepted Answer

2 decimal places

Question 4

A calculation yields $1.952447552 \div 1.485103868 = 1.314$. If the numbers have 8 and 9 significant figures respectively, how many significant figures should the answer have?

Accepted Answer

4 significant figures

Question 5

Which of the following is the correct result for $2.3357 	imes 10^6 + 6.92 	imes 10^5 + 3.0223 	imes 10^4$ expressed with the proper number of significant figures?

Accepted Answer

$3.030 	imes 10^6$

Question 6

Convert $0.0921 \ \mathrm{nm}$ to $\mathrm{pm}$.

Accepted Answer

$92.1 \ \mathrm{pm}$

Question 7

A healthy individual has a blood glucose concentration reported as $122 \ \mathrm{mg/dL}$. Convert that to units of $\mathrm{g/L}$.

Accepted Answer

$1.22 \ \mathrm{g/L}$

Question 8

A small hole in the wing of the space shuttle requires a $27.2 \ \mathrm{cm}^2$ patch. What is the patch's area in square inches ($\mathrm{in}^2$)? ($1 \ \mathrm{in} = 2.54 \ \mathrm{cm}$)

Accepted Answer

$4.22 \ \mathrm{in}^2$

Question 9

Pure gold has a density of $18.9 \ \mathrm{g/cm}^3$. Express this density in units of $\mathrm{lb/ft}^3$. ($1 \ \mathrm{lb} = 453.6 \ \mathrm{g}$, $1 \ \mathrm{ft}^3 = 2.54^3 	imes 10^3 \ \mathrm{cm}^3$)

Accepted Answer

$1181 \ \mathrm{lb/ft}^3$

Question 10

Which of the following best describes the rule for determining the number of significant figures in the result of a subtraction operation?

Accepted Answer

The result should have the same number of decimal places as the measurement with the fewest decimal places.

Question 11

If you multiply $0.088217 	imes 4.72$, how many significant figures should the answer have?

Accepted Answer

3 significant figures

Question 12

A scientist measures the mass of a sample as $1.852 \ \mathrm{g}$ and the volume as $0.025 \ \mathrm{L}$. What is the density in $\mathrm{g/L}$, reported with the correct number of significant figures?

Accepted Answer

$74.1 \ \mathrm{g/L}$

Question 13

Which of the following conversions is correct for $0.001317 \ \mathrm{kg}$ to $\mathrm{g}$?

Accepted Answer

$1.317 \ \mathrm{g}$

Question 14

A solution contains $0.00006000 \ \mathrm{mol}$ of solute in $0.001317 \ \mathrm{L}$ of solution. What is the molarity ($\mathrm{mol/L}$) of the solution?

Accepted Answer

$0.0456 \ \mathrm{mol/L}$

Question 15

Which of the following is the correct scientific notation for $0.00001871$?

Accepted Answer

$1.871 	imes 10^{-5}$

Question 16

A sample has a mass of $1471.00 \ \mathrm{g}$ and a volume of $808.0 \ \mathrm{cm}^3$. What is its density in $\mathrm{g/cm}^3$ with the correct number of significant figures?

Accepted Answer

$1.820 \ \mathrm{g/cm}^3$

Question 17

Which of the following is the correct conversion factor to use when converting $\mathrm{cm}^2$ to $\mathrm{in}^2$?

Accepted Answer

$1 \ \mathrm{in}^2 = 6.4516 \ \mathrm{cm}^2$

Question 18

A student records a measurement as $0.0588 \ \mathrm{mol}$, but the correct value is $0.061 \ \mathrm{mol}$. What is the percent error?

Accepted Answer

$3.6\%$

Question 19

Which of the following best describes the difference between accuracy and precision?

Accepted Answer

Accuracy refers to how close a measurement is to the true value, while precision refers to how close repeated measurements are to each other.

Significant Figures, Unit Conversions, and Scientific Calculations in General Chemistry 2.0

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