Textbook Question
Write balanced complete ionic and net ionic equations for each reaction.
a. K2SO4(aq) + CaI2(aq) → CaSO4(s) + KI(aq)
b. NH4Cl(aq) + NaOH(aq) → H2O(l) + NH3(g) + NaCl(aq)
c. AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
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Ch.4 - Chemical Quantities & Aqueous Reactions
Chapter 4, Problem 1
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) →
Verified step by step guidance1
Identify the type of reaction: Combustion reactions involve a substance reacting with oxygen to produce oxides, typically carbon dioxide and water.
For each reaction, write the unbalanced equation with the expected products: a. C(s) + O_2(g) → CO_2(g), b. C_3H_8O(l) + O_2(g) → CO_2(g) + H_2O(g), c. CS_2(s) + O_2(g) → CO_2(g) + SO_2(g), d. C_4H_6(g) + O_2(g) → CO_2(g) + H_2O(g).
Balance the carbon atoms first by ensuring the number of carbon atoms on the reactant side equals the number of carbon atoms in the carbon dioxide on the product side.
Next, balance the hydrogen atoms by adjusting the number of water molecules on the product side to match the hydrogen atoms in the reactants.
Finally, balance the oxygen atoms by adjusting the number of O_2 molecules on the reactant side to match the total number of oxygen atoms needed in the products.
Related Practice
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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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
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 _____ _____
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.