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Chapter 2: Problem 1

A compound is made up of entirely silicon and oxygen atoms. If there are 14.0 g of silicon and 32.0 g of oxygen present, what is the empirical formula of the compound? (A) \(\mathrm{SiO}_{2}\) (B) \(\mathrm{SiO}_{4}\) (C) \(\mathrm{Si}_{2} \mathrm{O}\) (D) \(\mathrm{Si}_{2} \mathrm{O}_{3}\)

Short Answer

Expert verified
The empirical formula of the compound will be \(\mathrm{SiO}_{4}\).

Step by step solution

01

Conversion to Moles

Firstly, convert the given masses of silicon and oxygen into moles. The atomic mass of silicon (Si) is approximately 28.1 g/mol, and for oxygen (O) it's 16.0 g/mol. Therefore, the number of moles of silicon is \(14.0 g / 28.1 g/mol = 0.50 mol\) and for oxygen \(32.0 g / 16.0 g/mol = 2.00 mol\).
02

Getting the Ratio

Next step is to get the simplest whole number ratio of the moles of silicon to moles of oxygen. This is done by dividing each by the smaller number of moles. Therefore the ratio of Si to O is \(0.50 mol / 0.50 mol : 2.00 mol / 0.50 mol = 1 : 4\).
03

Writing the empirical formula

Finally, the empirical formula of the compound is written. One silicon atom combines with four oxygen atoms. So the empirical formula of compound will be \(\mathrm{SiO}_{4}\).

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Most popular questions from this chapter

\(\mathrm{SF}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{SO}_{2}(g)+4 \mathrm{HF}(g) \Delta H=-828 \mathrm{kJ} / \mathrm{mol}\) Which of the following statements accurately describes the above reaction? (A) The entropy of the reactants exceeds that of the products. (B) \(\mathrm{H}_{2} \mathrm{O}(l)\) will always be the limiting reagent. (C) This reaction is never thermodynamically favored. (D) The temperature of the surroundings will increase as this reaction Progresses.

What is the general relationship between temperature and entropy for diatomic gases? (A) They are completely independent of each other; temperature has no effect on entropy. (B) There is a direct relationship, because at higher temperatures there is an increase in energy dispersal. (C) There is an inverse relationship, because at higher temperatures substances are more likely to be in a gaseous state. (D) It depends on the specific gas and the strength of the intermolecular forces between individual molecules.

The enthalpy values for several reactions are as follows: (I) \(\mathrm{CH}_{4}(g)+\mathrm{H}_{2}(g) \rightarrow \mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g)\) \(\quad \Delta H=-131 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) (II) \(\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow 3 \mathrm{H}_{2}(g)+\mathrm{CO}(g)\) \(\quad \Delta H=206 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) (III) \(\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)\) \(\quad \Delta H=-41 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) (IV) \(\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) \(\quad \Delta H=-890 \mathrm{kJ} / \mathrm{mol}_{\mathrm{rxn}}\) In which of the reactions does the amount of energy released by the formation of bonds in the products exceed the amount of energy necessary to break the bonds of the reactants by the greatest amount? (A) Reaction I (B) Reaction II (C) Reaction III (D) Reaction IV

A solution of sulfurous acid, \(\mathrm{H}_{2} \mathrm{SO}_{3}\) , is present in an aqueous solution. Which of the following represents the concentrations of three different ions in solution? (A) \(\left[\mathrm{SO}_{3}^{2-}\right]>\left[\mathrm{HSO}_{3}^{-}\right]>\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]\) (B) \(\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]>\left[\mathrm{HSO}_{3}^{-}\right]>\left[\mathrm{SO}_{3}^{2-}\right]\) (C) \(\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]>\left[\mathrm{HSO}_{3}^{-}\right]=\left[\mathrm{SO}_{3}^{2-}\right]\) (D) \(\left[\mathrm{SO}_{3}^{2-}\right]=\left[\mathrm{HSO}_{3}^{-}\right]>\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]\)

20.0 \(\mathrm{mL}\) of 1.0 \(\mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3}\) is placed in a beaker and titrated with a solution of \(1.0 \mathrm{M} \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2},\) resulting in the creation of a precipitate. If the experiment were repeated and the \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) was diluted to 40.0 \(\mathrm{mL}\) with distilled water prior to the titration, how would that affect the volume of \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) needed to reach the equivalence point? (A) It would be cut in half. (B) It would decrease by a factor of 1.5. (C) It would double. (D) It would not change.
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