Explain whether the given statement is correct concerning sorbic acid, $\mathrm{C}_6 \mathrm{H}_8 \mathrm{O}_2$, an inhibitor of mould and yeast.

It has a $\mathrm{C}: \mathrm{H}$ : $\mathrm{O}$ mass ratio of $3: 4: 1$

Explain whether the given statement is correct concerning glucose (blood sugar), $\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6$:

The highest percentage, by mass, is that of $\mathrm{H}$

Explain whether the given statement is correct concerning glucose (blood sugar), $\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6$:

The proportions, by mass, of $\mathrm{C}$ and $\mathrm{O}$ are equal

Explain whether the given statement is correct concerning glucose (blood sugar), $\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6$:

The ratio of $\mathrm{C}: \mathrm{H}: \mathrm{O}$ atoms is the same as in dihydroxyacetone, $\left(\mathrm{CH}_2 \mathrm{OH}\right)_2 \mathrm{CO}$

Explain whether the given statement is correct concerning glucose (blood sugar), $\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6$:

The percentages, by mass, of $\mathrm{C}$ and $\mathrm{O}$ are the same as in $\mathrm{CO}$.

Figure shows the conductivity test for sulfuric acid. A similar result is observed for barium hydroxide. (a) How would Arrhenius explain these observations?

(b) Write the chemical equation for the neutralization of sulfuric acid by barium hydroxide. Consult the solubility table to determine the state of the ionic product.

(c) Figure 10(b) shows the final mixture produced when sulfuric acid is completely neutralized by barium hydroxide. Why is there a difference in conductivity? What would be observed if sodium hydroxide were used instead? Why? completely neutralized with barium hydroxide, the resulting moxture does not conduct electricity, and the bulb no longer lights up.

Appendix E describes a useful study aid known as concept mapping. Using the method presented in Appendix E, construct a concept map illustrating the different concepts in Sections 3-2 and 3-3.

Appendix E describes a useful study aid known as concept mapping. Using the method presented in Appendix E, construct a concept map illustrating the different concepts in Sections 3-2 and 3-3.

Ibuprofen is a compound used in painkillers. When a $2.174 \mathrm{~g}$ sample is burned in an excess of oxygen, it yields $6.029 \mathrm{~g} \mathrm{CO}_2$ and $1.709 \mathrm{~g} \mathrm{H}_2 \mathrm{O}$ as the sole products. What is the empirical formula of ibuprofen?

Ibuprofen is a compound used in painkillers. When a $2.174 \mathrm{~g}$ sample is burned in an excess of oxygen, it yields $6.029 \mathrm{~g} \mathrm{CO}_2$ and $1.709 \mathrm{~g} \mathrm{H}_2 \mathrm{O}$ as the sole products. What is the percent composition, by mass, of ibuprofen?

Determine the mass, in grams, of a quantity of the amino acid lysine, $\mathrm{C}_6 \mathrm{H}_{14} \mathrm{~N}_2 \mathrm{O}_2$, containing $3.03 \mathrm{~mol} \mathrm{~N}$ atoms

The hemoglobin content of blood is about $15.5 \mathrm{~g} / 100 \mathrm{~mL}$ blood. The molar mass of hemoglobin is about $64,500 \mathrm{~g} / \mathrm{mol}$, and there are four iron (Fe) atoms in a hemoglobin molecule. Approximately how many Fe atoms are present in the $6 \mathrm{~L}$ of blood in a typical adult?

Learning goal is to analyze the experiment used to determine the properties of an electron. In 1909, Robert Milikan performed an experiment involving tiny, charged drops of oil. The drops were charged because they had picked up extra electrons. Millikan was able to measure the charge on each drop in coulombs. Here is an example of what his data may have looked like:

In Milikan's experiment, the charge on each drop of oil was measured in coulombs. Imagine the same experiment, but with charges measured in a fictitious unit called a zeet (Z).

What is the charge on an electron in zeets?

Determine the mass, in grams, of $4.03 \times 10^{24}$ molecules of stearic acid, $\mathrm{C}_{18} \mathrm{H}_{36} \mathrm{O}_2$