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Chapter 1: Problem 11

A sample of a compound known to consist of only carbon, hydrogen, and oxygen is found to have a total mass of 29.05 g. If the mass of the carbon is 18.02 g and the mass of the hydrogen is 3.03 g, what is the empirical formula of the compound? (A) \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}\) (B) \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\) (C) \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{3}\) (D) \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}_{2}\)

Short Answer

Expert verified
The empirical formula of the compound is \( \mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\), so the answer is (B).

Step by step solution

01

Calculate the Number of Moles of Each Element

To begin, calculate the number of moles of carbon, hydrogen, and oxygen in the sample. The molar mass of carbon, hydrogen, and oxygen is approximately 12 g/mol, 1 g/mol, and 16 g/mol respectively. Therefore, the moles of carbon, hydrogen, and oxygen are 18.02 g \( \div \) 12 g/mol = 1.50 mol (for carbon), 3.03 g \( \div \) 1 g/mol = 3.03 mol (for hydrogen), and for the oxygen, first subtract the mass of carbon and hydrogen from the total mass to get the mass of oxygen: 29.05 g - 18.02 g - 3.03 g = 8 g. Hence, the moles of oxygen is 8 g \( \div \) 16 g/mol = 0.50 mol.
02

Determine the Empirical Formula

The empirical formula gives the ratio of the number of atoms in a compound. Here, the mole ratio is 1.50 : 3.03 : 0.50. You can simplify this ratio by dividing all the elements by the smallest value, which is 0.50. This gives a ratio of 3 : 6 : 1. However, it is customary to use whole numbers in empirical formulas, so we need to simplify the ratio further. Dividing 3 : 6 : 1 by the greatest common factor, which is 3, we obtain the ratio 1 : 2 : 1/3. Multiplying all numbers by 3 to get to a whole number for oxygen, we get the ratio 3 : 6 : 1.
03

Match the Formula

Finally, you match the ratios obtained with the options given. The empirical formula with the ratio 3 : 6 : 1 corresponds to (B) \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\) .

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Most popular questions from this chapter

During a chemical reaction, NO(g) gets reduced and no nitrogen- containing compound is oxidized. Which of the following is a possible product of this reaction? (A) \(\mathrm{NO}_{2}(g)\) (B) \(\mathrm{N}_{2}(g)\) (C) \(\mathrm{NO}_{3}^{-}(a q)\) (D) \(\mathrm{NO}_{2}^{-}(a q)\)

$$2 \mathrm{NOCl} \rightarrow 2 \mathrm{NO}+\mathrm{Cl}_{2}$$ The reaction above takes place with all of the reactants and products in the gaseous phase. Which of the following is true of the relative rates of disappearance of the reactants and appearance of the products? (A) NO appears at twice the rate that NOCl disappears. (B) NO appears at the same rate that NOCl disappears. (C) NO appears at half the rate that NOCl disappears. (D) \(\mathrm{Cl}_{2}\) appears at the same rate that NOCl disappears.

Questions 32-36 refer to the following. Two half-cells are set up as follows: Half-Cell A: Strip of \(\mathrm{Cu}(s)\) in \(\mathrm{CuNO}_{3}(a q)\) Half-Cell B: Strip of \(\mathrm{Zn}(s)\) in \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}\) (aq) When the cells are connected according to the diagram below, the following reaction occurs: GRAPH CAN'T COPY $$2 \mathrm{Cu}^{+}(a q)+\mathrm{Zn}(s) \rightarrow 2 \mathrm{Cu}(s)+\mathrm{Zn}^{2+}(a q) E^{\circ}=+1.28 \mathrm{V}$$ What will happen in the salt bridge as the reaction progresses? (A) The Na' ions will flow to the Cu/Cu' half-cell. (B) The Br' ions will flow to the Cu/Cu' half-cell. (C) Electrons will transfer from the Cu/Cu' half-cell to the Zn/Zn" half cell. (D) Electrons will transfer from the \(\mathrm{Zn} / \mathrm{Zn}^{2+}\) half- cell to the Cu/Cu' half cell.

Questions 32-36 refer to the following. Two half-cells are set up as follows: Half-Cell A: Strip of \(\mathrm{Cu}(s)\) in \(\mathrm{CuNO}_{3}(a q)\) Half-Cell B: Strip of \(\mathrm{Zn}(s)\) in \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}\) (aq) When the cells are connected according to the diagram below, the following reaction occurs: GRAPH CAN'T COPY $$2 \mathrm{Cu}^{+}(a q)+\mathrm{Zn}(s) \rightarrow 2 \mathrm{Cu}(s)+\mathrm{Zn}^{2+}(a q) E^{\circ}=+1.28 \mathrm{V}$$ How many moles of electrons must be transferred to create 127 g of copper? (A) 1 mole of electrons (B) 2 moles of electrons (C) 3 moles of electrons (D) 4 moles of electrons

A laboratory technician wishes to create a buffered solution with a pH of 5. Which of the following acids would be the best choice for the buffer? (A) \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4} \quad K_{a}=5.9 \times 10^{-2}\) (B) \(\mathrm{H}_{3} \mathrm{AsO}_{4} \quad K_{a}=5.6 \times 10^{-3}\) (C) \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2} \quad K_{a}=1.8 \times 10^{-5}\) (D) \(\mathrm{HOCl}\) \(\quad K_{a}=3.0 \times 10^{-8}\)
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