Textbook Question
Write balanced complete ionic and net ionic equations for each reaction.
c. NaOH(aq) + HC2H3O2(aq) → H2O(l ) + NaC2H3O2(aq)
d. Na3PO4(aq) + NiCl2(aq) → Ni3(PO4)2(s) + NaCl(aq)
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Ch.4 - Chemical Quantities & Aqueous Reactions
Chapter 4, Problem 3
Consider the balanced equation: 2 N2H4(g) + N2O4(g) → 3 N2(g) + 4 H2O(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. Mol N2H4 Mol N2O4 Mol N2 Mol H2O 2 _____ _____ _____ _____ 5 _____ _____ _____ _____ _____ 10 _____ _____ 11.8 _____ 2.5 _____ _____ _____ _____ 4.2 _____ _____
Verified step by step guidance1
Identify the stoichiometric coefficients from the balanced equation: 2 N2H4(g) + 1 N2O4(g) → 3 N2(g) + 4 H2O(g).
Use the stoichiometric coefficients to set up mole ratios for each reactant and product. For example, the mole ratio of N2H4 to N2 is 2:3, and the mole ratio of N2O4 to H2O is 1:4.
For each row in the table, use the given number of moles to calculate the unknowns using the mole ratios. For instance, if 2 moles of N2H4 are given, calculate the moles of N2O4 needed and the moles of N2 and H2O produced.
If the number of moles of a product is given, use the inverse of the mole ratios to find the required moles of reactants. For example, if 11.8 moles of N2 are produced, calculate the moles of N2H4 and N2O4 required.
Repeat the process for each row, ensuring that the stoichiometric relationships are maintained throughout the calculations.
Related Practice
Textbook Question
Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) → FeCl2(s) + H2S(g) A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?
Open Question
Complete and balance each combustion reaction equation: a. C(s) + O2(g) → b. C3H8O(l) + O2(g) → c. CS2(s) + O2(g) → d. C4H6(g) + O2(g) →
Open Question
We prepare a solution by mixing 0.10 L of 0.12 M sodium chloride with 0.23 L of a 0.18 M MgCl2 solution. What volume of a 0.20 M silver nitrate solution is needed to precipitate all the Cl- ions in the solution as AgCl?
Open Question
Consider the unbalanced equation for the combustion of hexane: C6H14(g) + O2(g) → CO2(g) + H2O(g). Balance the equation and determine how many moles of O2 are required to react completely with 7.2 moles of C6H14.
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 0.461 mole of HC2H3O2.
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