In each row check off the boxes that apply to the highlighted reactant. reaction Fe³*(aq) + 6 H₂O(1) → Fe(H₂0)³† (aq) 3+ HCN(aq) + CH,NH,(aq) → CN (aq) + CH,NH,(aq) Ni(s) + 4 CO(g) → Ni(CO) 4(1) The highlighted reactant acts as a... (check all that apply) Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base

In each row check off the boxes that apply to the highlighted reactant. reaction Fe³*(aq) + 6 H₂O(1) → Fe(H₂0)³† (aq) 3+ HCN(aq) + CH,NH,(aq) → CN (aq) + CH,NH,(aq) Ni(s) + 4 CO(g) → Ni(CO) 4(1) The highlighted reactant acts as a... (check all that apply) Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 125QRT: A student set up an experiment for six different trials of the reaction between 1.00-M aqueous...

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You are given mixtures containing the following compounds. Which compound in each pair could be separated by stirring the solid mixture with water? (a) NaOH and Ca(OH)2 (b) MgC12 and MgF2 (c) AgI and KI (d) NH4Cl and PbCl2
A student set up an experiment for six different trials of the reaction between 1.00-M aqueous acetic acid, CH3COOH, and solid sodium hydrogen carbonate, NaHCO3. CH3COOH(aq) + NaHCO3(s) NaCH3CO2(aq) + CO2(g) + H2O() The volume of acetic acid was kept constant, but the mass of sodium bicarbonate increased with each trial. The results of the tests are shown in the figure. (a) In which trial(s) is the acetic acid the limiting reactant? (b) In which trial(s) is sodium bicarbonate the limiting reactant? (c) Explain your reasoning in parts (a) and (b).
13. Complete the table below. Equation 1: Equation 2: 1 - H₂(g) + O2(g) → H₂0 (1) Mg(s) + 2HCl(aq) → MgCl2(aq) + H₂(g) Equation 3:P MgO(s) + 2HCl(aq) MgO(s) + 2HCl(aq) → MgCl2(aq) + H₂0 (1) H₂O(1) AH₂ = -285.8 kJ AH3 = ΔΗ, = teori
In each row check off the boxes that apply to the highlighted reactant. reaction Ni(s) + 4CO (g) → Ni(CO) 4(1) 3+ 3+ Al³+ (aq) + 6H₂O(1) → Al(H₂0)³+ (aq) + HBr(aq) + NH3(aq) · → Br_(aq) + NH4(aq) The highlighted reactant acts as a... (check all that apply) ооо 0 0 0 0 00 00 о Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base Brønsted-Lowry acid Brønsted-Lowry base Lewis acid Lewis base X Ś
Classify each of these reactions. Reaction 2 NaOH(aq) + Pb(CIO3)₂(aq) - C₂H₂(g) + 30₂(g) - 2 AgNO3(aq) + Zn(s) HI(aq) + LiOH(aq) 2 NaC1O3(aq) + Pb(OH)₂ (s) 2 CO₂(g) + 2 H₂O(1) Zn(NO3)₂(aq) + 2 Ag(s) H₂O(1) + Lil(aq) redox Answer Bank acid-base neutralization Type precipitation
Classify each of these reactions. Pb(NO3)₂(aq) + 2 KCl(aq) CH₂(g) + 2O₂(g) → CO₂(g) + 2 H₂O(1) Cu(s) + FeCl₂(aq) Fe(s) + CuCl₂ (aq) 2 KOH(aq) + H₂SO4 (aq) → K₂SO4 (aq) + 2 H₂O(1) - redox PbCl₂ (s) + 2 KNO3(aq) Answer Bank acid-base neutralization precipitation
Classify each chemical reaction: KOH(aq) + HBrO (aq) reaction K BrO (aq) + H₂O (1) Na Cl (aq) + AgNO3(aq) → NaNO3(aq) + Ag Cl (s) 16K (s) + S₂ (s)→ 8K₂S (s) 2CH₂CH₂CO₂H (1) + 70₂(g) → 6CO₂(g) + 6H₂O(g) ✓ 6 ✓ 7 type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition ✓8 X precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base 9 10
Classify each chemical reaction: 2K (s) + Br₂ (1) 2K Br(s) FeSO₂ (aq) + PbCl₂ (aq) → FeCl₂ (aq) + PbSO₂ (s) reaction 2CH₂CH₂(g) +70, (g) 4CO₂(g) + 6H₂O(g) KOH(aq) + HBrO (aq) → KBrO(aq) + H₂O(1) Explanation Recheck type of reaction (check all that apply) combination O single replacement Odouble replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination precipitation combustion acid-base X precipitation combustion acid-base precipitation combustion acid-base Oprecipitation combustion O single replacement O double replacement acid-base O decomposition MacBook Air S © 2023 McGraw Hill LLC. All Rights Resea
- Classify each reaction in as many ways as possible. (a) 2 Al(s) + 3 Cu(NO3)2(aq) – 2 Al(NO3)3(aq) + 3Cu(s) (b) HBr(aq) + KHSO3(aq) H2O(1) + SO2(g) + NaBr(aq) → H,S(g) + 2Nal(aq) (а) К,СО,(ag) + FeBrz(aq) — FeCO,(6) + 2KBr(ag) (c) 2 HI(aq) + Na,S(aq)
1) Match the each of the following chemical equations with the correct type of reaction(s). CH4 (9) + 2O₂(g) → CO₂(g) + 2 H₂O(g) Cu²+ (aq) + S²(aq) → CuS(s) 2 HC₂H3O₂(aq) + Ba(OH)₂ (aq) 2 LiCl(aq) + Sr(NO3)2(aq) → 2 LiNO3(aq) + SrCl₂(aq) → 2 H₂O(l) + Ba(C₂H302)2(aq) Select One Select One Select One Select One: O 6
2 Ag(s) + ¿ O2(g) + 2 H†(aq) 2 Ag*(aq) + H20(1) +1.23 O2(g) + 4 H*(aq) + 4 e¯ → 2 H2O(I) - +1.06 Br2(1) + 2 e¯ → 2 Br¯(aq) - +0.96 NO3¯(aq) + 4 H*(aq) + 3 e¯ NO(g) + 2 H2O(1) +0.80 Ag*(aq) + e-→ Ag(s) Now what are the values of E°, cell, AG°, and K?
Let us assume that Fe(OH)3(s)Fe(OH)3(s) is completely insoluble, which signifies that the precipitation reaction with NaOH(aq)NaOH(aq) (presented in the transition) would go to completion. Fe3+(aq)+3NaOH(aq) → Fe(OH)3(s)+3Na+(aq)Fe3+(aq)+3NaOH(aq) → Fe(OH)3(s)+3Na+(aq) If you had a 0.250 L solution containing 0.0140 M of Fe3+(aq), and you wished to add enough 1.37 M NaOH(aq) NaOH(aq) to precipitate all of the metal, what is the minimum amount of the NaOH(aq) solution you would need to add? Assume that the NaOH(aq) solution is the only source of OH−(aq) for the precipitation. Express the volume to three significant figures and include the appropriate units.