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 91a,d
Complete and balance each gas-evolution equation. a. HBr(aq) + NiS(s) → d. HClO4(aq) + Li2CO3(aq) →
Verified step by step guidance1
Step 1: Identify the reactants and products for each reaction. For reaction (a), the reactants are HBr(aq) and NiS(s). For reaction (d), the reactants are HClO_4(aq) and Li_2CO_3(aq).
Step 2: Determine the type of reaction. Both reactions are gas-evolution reactions, which typically involve the formation of a gas as one of the products.
Step 3: Predict the products. For reaction (a), HBr reacts with NiS to form H_2S(g) and NiBr_2(aq). For reaction (d), HClO_4 reacts with Li_2CO_3 to form CO_2(g), H_2O(l), and LiClO_4(aq).
Step 4: Write the unbalanced chemical equations. For reaction (a), it is HBr(aq) + NiS(s) → H_2S(g) + NiBr_2(aq). For reaction (d), it is HClO_4(aq) + Li_2CO_3(aq) → CO_2(g) + H_2O(l) + LiClO_4(aq).
Step 5: Balance each equation by adjusting coefficients to ensure the same number of each type of atom on both sides of the equation. Start with the most complex molecule and balance elements one at a time, checking each element as you proceed.
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
Complete and balance each gas-evolution equation. b. HCl(aq) + KHCO3(aq) → c. HC2H3O2(aq) + NaHSO3(aq) → d. (NH4)2SO4(aq) + Ca(OH)2(aq) →
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
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 _____ _____