Textbook Question
Write the balanced chemical equation for the reaction of aqueous potassium hydroxide with aqueous iron(III) chloride to form solid iron(III) hydroxide and aqueous potassium chloride.
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Ch.4 - Chemical Reactions and Chemical Quantities
Chapter 4, Problem 33a
Balance the equation and calculate how many moles of O2 form when each quantity of reactant completely reacts. N2O5( g) → NO2(g) + O2(g) a. 1.2 mol N2O5
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Balancing Chemical Equations
Balancing chemical equations is essential to ensure that the number of atoms for each element is the same on both sides of the equation. This reflects the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. In the given reaction, N2O5 decomposes into NO2 and O2, and balancing the equation will help determine the stoichiometric relationships between the reactants and products.
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Balancing Chemical Equations
Stoichiometry
Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. It allows chemists to predict how much of a product will form from a given amount of reactant. In this case, once the equation is balanced, stoichiometric coefficients can be used to determine the moles of O2 produced from the moles of N2O5 that react.
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Mole Concept
The mole concept is a fundamental principle in chemistry that relates the mass of a substance to the number of particles it contains. One mole of any substance contains Avogadro's number (approximately 6.022 x 10^23) of entities, whether they are atoms, molecules, or ions. Understanding this concept is crucial for converting between moles and grams, and for calculating the amount of O2 produced in the reaction based on the initial moles of N2O5.
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Related Practice
Textbook Question
Balance each chemical equation. b. Co(NO3)3(aq) + (NH4)2S(aq) → Co2S3(s) + NH4NO3(aq)
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Textbook Question
Consider the unbalanced equation for the neutralization of acetic acid: HC2H3O2(aq) + Ba(OH)2(aq) → H2O(l) + Ba(C2H3O2)2(aq) Balance the equation and determine how many moles of Ba(OH)2 are required to completely neutralize 1.22 mol of HC2H3O2.
Textbook Question
Balance the equation and calculate how many moles of N2 form when each quantity of reactant completely reacts. N2H4(l) → NH3(g) + N2(g) c. 33.9 g N2H4
Textbook Question
Consider the balanced equation:
SiO2(s) + 3 C(s) → SiC(s) + 2 CO(g)
Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms.
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Textbook Question
Hydrobromic acid dissolves solid iron according to the reaction:
Fe(s) + 2 HBr(aq) → FeBr2(aq) + H2(g)
What mass of HBr (in g) do you need to dissolve a 2.80-g pure iron bar on a padlock? What mass of H2 would the complete reaction of the iron bar produce?