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Chapter 3: Problem 56

What parts of balanced chemical equations give information about the relative numbers of moles of reactants and products involved in a reaction?

Short Answer

Expert verified
The stoichiometric coefficients in a balanced chemical equation give information about the relative numbers of moles of reactants and products involved in a reaction. These coefficients are the numbers written in front of each species participating in the reaction and ensure that the number of atoms of each element is equal on both sides of the reaction, obeying the law of conservation of mass. The stoichiometric coefficients represent the relative moles of reactants and products, allowing us to calculate the amounts needed for or produced in the reaction. For example, in the equation CH4 + 2O2 -> CO2 + 2H2O, the coefficients indicate that 1 mole of CH4 reacts with 2 moles of O2 to produce 1 mole of CO2 and 2 moles of H2O.

Step by step solution

01

Balanced Chemical Equation

A balanced chemical equation is a representation of a chemical reaction in which the number of atoms of each element in both the reactants and the products are the same. Balanced chemical equations obey the law of conservation of mass, which states that matter cannot be created or destroyed. Example of a balanced chemical equation: CH4 + 2O2 -> CO2 + 2H2O
02

Identification of Reactants and Products

In a balanced chemical equation, the reactants are written on the left side of the reaction, while the products are written on the right side of the reaction. The arrow symbol (->) separates reactants from products. In the given example, CH4 (Methane) and 2O2 (Oxygen) are the reactants and CO2 (Carbon dioxide) and 2H2O (Water) are the products.
03

Stoichiometric Coefficients

Stoichiometric coefficients are the numbers written in front of each species participating in the reaction, which denote their relative amounts. These coefficients are used to balance the equation, ensuring that the number of atoms of each element is equal on both sides of the reaction. In the given example, the stoichiometric coefficients are: 1 (for CH4), 2 (for O2), 1 (for CO2), and 2 (for H2O).
04

Relative Moles of Reactants and Products

The stoichiometric coefficients give information about the relative number of moles of reactants and products involved in the reaction. A balanced chemical equation conveys the stoichiometric relationship between reactants and products, which allows us to calculate the amount of each substance needed for the reaction or the amount of each substance produced in the reaction. In the given example, the stoichiometric coefficients indicate that: - 1 mole of CH4 reacts with 2 moles of O2. - 1 mole of CO2 is produced. - 2 moles of H2O are produced. The stoichiometric coefficients (relative number of moles) are the parts of the balanced chemical equations that give information about the relative numbers of moles of reactants and products involved in a reaction.

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Most popular questions from this chapter

What is the molecular formula of each of the following compounds? (a) empirical formula \(\mathrm{HCO}_{2}\), molar mass \(=90.0 \mathrm{~g} / \mathrm{mol}\) (b) empirical formula \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}\), molar mass \(=88 \mathrm{~g} / \mathrm{mol}\)

A chemical plant uses electrical energy to decompose aqueous solutions of \(\mathrm{NaCl}\) to give \(\mathrm{Cl}_{2}, \mathrm{H}_{2}\), and \(\mathrm{NaOH}\) : \(2 \mathrm{NaCl}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \underset{2 \mathrm{NaOH}(a q)}{\longrightarrow}+\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g)\) If the plant produces \(1.5 \times 10^{6} \mathrm{~kg}\left(1500\right.\) metric tons) of \(\mathrm{Cl}_{2}\) daily, estimate the quantities of \(\mathrm{H}_{2}\) and \(\mathrm{NaOH}\) produced.

Detonation of nitroglycerin proceeds as follows: \(4 \mathrm{C}_{3} \mathrm{H}_{5} \mathrm{~N}_{3} \mathrm{O}_{9}(l)\) $$ 12 \mathrm{CO}_{2}(g)+6 \mathrm{~N}_{2}(g)+\mathrm{O}_{2}(g)+10 \mathrm{H}_{2} \mathrm{O}(g) $$ (a) If a sample containing \(2.00 \mathrm{~mL}\) of nitroglycerin (density \(=1.592 \mathrm{~g} / \mathrm{mL}\) ) is detonated, how many total moles of gas are produced? (b) If each mole of gas occupies \(55 \mathrm{~L}\) under the conditions of the explosion, how many liters of gas are produced? (c) How many grams of \(\mathrm{N}_{2}\) are produced in the detonation?

(a) Define the terms limiting reactant and excess reactant. (b) Why are the amounts of products formed in a reaction determined only by the amount of the limiting reactant? (c) Why should you base your choice of what compound is the limiting reactant on its number of initial moles, not on its initial mass in grams?

Very small crystals composed of 1000 to 100,000 atoms, called quantum dots, are being investigated for use in electronic devices. (a) A quantum dot was made of solid silicon in the shape of a sphere, with a diameter of \(4 \mathrm{~nm}\). CalcuJate the mass of the quantum dot, using the density of silicon \(\left(23 \mathrm{~g} / \mathrm{cm}^{3}\right)\). (b) How many silicon atoms are in the quantum dot? (c) The density of germanium is \(5.325 \mathrm{~g} / \mathrm{cm}^{3}\). If you made a \(4 \mathrm{~nm}\) quantum dot of germanium, how many Ge atoms would it contain? Assume the dot is spherical
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