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Chapter 3: Problem 106

How many moles of \(\mathrm{O}\) are needed to combine with 0.212 mole of \(\mathrm{C}\) to form (a) \(\mathrm{CO}\) and (b) \(\mathrm{CO}_{2}\) ?

Short Answer

Expert verified
(a) 0.212 mole of \(\mathrm{O}\) (b) 0.424 mole of \(\mathrm{O}\)

Step by step solution

01

Balancing the chemical equation for formation of CO

The chemical equation for the formation of \(\mathrm{CO}\) from \(\mathrm{C}\) and \(\mathrm{O}\) is given by \(\mathrm{C} + \mathrm{O} \rightarrow \mathrm{CO}\). This equation is already balanced, so no additional steps are needed. The stoichiometric coefficient in front of \(\mathrm{C}\) and \(\mathrm{O}\) is 1, meaning that one mole of \(\mathrm{C}\) reacts with one mole of \(\mathrm{O}\) to form one mole of \(\mathrm{CO}\).
02

Calculating the moles of O needed to form CO

Given that the molar ratio of \(\mathrm{C}\) to \(\mathrm{O}\) is 1:1 in the formation of \(\mathrm{CO}\), the moles of \(\mathrm{O}\) needed to react with 0.212 mole of \(\mathrm{C}\) is also 0.212 mole.
03

Balancing the chemical equation for formation of CO2

The chemical equation for the formation of \(\mathrm{CO}_{2}\) from \(\mathrm{C}\) and \(\mathrm{O}\) is given by \(\mathrm{C} + \mathrm{O}_{2} \rightarrow \mathrm{CO}_{2}\). This equation is also balanced. The stoichiometric coefficient in front of \(\mathrm{C}\) and \(\mathrm{O}_{2}\) is 1, meaning that one mole of \(\mathrm{C}\) reacts with one mole of \(\mathrm{O}_{2}\) to form one mole of \(\mathrm{CO}_{2}\). Since \(\mathrm{O}_{2}\) is a diatomic molecule, one mole of \(\mathrm{O}_{2}\) contains two moles of \(\mathrm{O}\). Thus, one mole of \(\mathrm{C}\) reacts with two moles of \(\mathrm{O}\) to form one mole of \(\mathrm{CO}_{2}\).
04

Calculating the moles of O needed to form CO2

Given that the molar ratio of \(\mathrm{C}\) to \(\mathrm{O}\) is 1:2 in the formation of \(\mathrm{CO}_{2}\), two times the given moles of \(\mathrm{C}\) will be the moles of \(\mathrm{O}\) needed. This means that 2 * 0.212 mole = 0.424 mole of \(\mathrm{O}\) needed to react with 0.212 mole of \(\mathrm{C}\) to form \(\mathrm{CO}_{2}\).

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Most popular questions from this chapter

One of the reactions that occurs in a blast furnace, where iron ore is converted to cast iron, is$$\mathrm{Fe}_{2} \mathrm{O}_{3}+3 \mathrm{CO} \longrightarrow 2 \mathrm{Fe}+3 \mathrm{CO}_{2}$$Suppose that \(1.64 \times 10^{3} \mathrm{~kg}\) of \(\mathrm{Fe}\) are obtained from a \(2.62 \times 10^{3} \mathrm{~kg}\) sample of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\). Assuming that the reaction goes to completion, what is the percent purity of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) in the original sample?

Peroxyacylnitrate (PAN) is one of the components of smog. It is a compound of \(\mathrm{C}, \mathrm{H}, \mathrm{N},\) and \(\mathrm{O} .\) Determine the percent composition of oxygen and the empirical formula from the following percent composition by mass: 19.8 percent \(\mathrm{C}, 2.50\) percent \(\mathrm{H}, 11.6\) percent \(\mathrm{N}\). What is its molecular formula given that its molar mass is about \(120 \mathrm{~g}\) ?

If we know the empirical formula of a compound, what additional information do we need to determine its molecular formula?

Write balanced equations for the following reactions described in words. (a) Pentane burns in oxygen to form carbon dioxide and water. (b) Sodium bicarbonate reacts with hydrochloric acid to form carbon dioxide, sodium chloride, and water. (c) When heated in an atmosphere of nitrogen, lithium forms lithium nitride. (d) Phosphorus trichloride reacts with water to form phosphorus acid and hydrogen chloride. (e) Copper(II) oxide heated with ammonia will form copper, nitrogen gas, and water.

(a) For molecules having small molecular masses, mass spectrometry can be used to identify their formulas. To illustrate this point, identify the molecule that most likely accounts for the observation of a peak in a mass spectrum at 16 amu, 17 amu, 18 amu, and 64 amu. (b) Note that there are (among others) two likely molecules that would give rise to a peak at 44 amu, namely, \(\mathrm{C}_{3} \mathrm{H}_{8}\) and \(\mathrm{CO}_{2} .\) In such cases, a chemist might try to look for other peaks generated when some of the molecules break apart in the spectrometer. For example, if a chemist sees a peak at 44 amu and also one at 15 amu, which molecule is producing the 44 -amu peak? Why? (c) Using the following precise atomic masses \(-\mathrm{H}\) ( 1.00797 amu), \({ }^{12} \mathrm{C}(12.00000 \mathrm{amu}),\) and \({ }^{16} \mathrm{O}(15.99491 \mathrm{amu})-\) how precisely must the masses of \(\mathrm{C}_{3} \mathrm{H}_{8}\) and \(\mathrm{CO}_{2}\), be measured to distinguish between them?
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